Calcium Phosphate Precipitation (Bone Mineral)

3CaCl₂ + 2Na₃PO₄ → Ca₃(PO₄)₂↓ + 6NaCl

Descripción general

Calcium chloride reacts with trisodium phosphate to form a white precipitate of calcium phosphate (Ksp = 2.1 × 10⁻³³). Calcium phosphate, particularly the hydroxyapatite form Ca₅(PO₄)₃OH, is the primary mineral component of bones and teeth. It accounts for about 70% of bone mass.

Participantes

Rol	Sustancia	Coeficiente	Estado
Producto	Sodium Chloride NaCl	6	(aq)

Ejemplo cotidiano

Your bones and teeth are built from a form of calcium phosphate. Maintaining adequate calcium and phosphorus intake keeps this mineral being deposited.

Importancia industrial

El fosfato de calcio se utiliza en injertos óseos e implantes dentales, como suplemento alimentario, en cerámicas y como materia prima para la producción de ácido fosfórico.

Propiedades

Tipo: Precipitation
Reversible: No
Energía: Exotérmico
ΔH: -105,0 kJ/mol

Reacciones relacionadas

Aluminum Hydroxide Precipitation Barium Carbonate Precipitation Barium Sulfate Precipitation Cadmium Sulfide Precipitation (Yellow) Calcium Fluoride Precipitation (Fluorite) Chromium(III) Hydroxide Precipitation Lead Carbonate Precipitation Lead Chloride Precipitation Calcium Carbonate Precipitation Iron(III) Hydroxide Precipitation

Frequently Asked Questions

What is the equation for Calcium Phosphate Precipitation (Bone Mineral)?

The balanced equation is: 3CaCl₂ + 2Na₃PO₄ → Ca₃(PO₄)₂↓ + 6NaCl.

What type of reaction is Calcium Phosphate Precipitation (Bone Mineral)?

Calcium Phosphate Precipitation (Bone Mineral) is a precipitation reaction.

Is Calcium Phosphate Precipitation (Bone Mineral) exothermic or endothermic?

Calcium Phosphate Precipitation (Bone Mineral) is exothermic (releases energy). The enthalpy change (ΔH) is -105.0 kJ/mol.