Calcium Phosphate Precipitation (Bone Mineral)

3CaCl₂ + 2Na₃PO₄ → Ca₃(PO₄)₂↓ + 6NaCl

Visão geral

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

Papel	Substância	Coeficiente	Estado
Produto	Sodium Chloride NaCl	6	(aq)

Exemplo do cotidiano

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

Importância industrial

O fosfato de cálcio é utilizado em enxertos ósseos e implantes dentários, como suplemento alimentar, em cerâmicas e como matéria-prima para a produção de ácido fosfórico.

Propriedades

Tipo: Precipitation
Reversível: Não
Energia: Exotérmico
ΔH: -105,0 kJ/mol

Reações 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.