Calcium Phosphate Precipitation (Bone Mineral)

3CaCl2 + 2Na3PO4 → Ca3(PO4)2↓ + 6NaCl

Übersicht

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.

Teilnehmer

Rolle Substanz Koeffizient Zustand
Produkt Sodium Chloride NaCl 6 (aq)

Alltägliches Beispiel

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

Industrielle Bedeutung

Calcium phosphate is used in bone grafts and dental implants, as a food supplement, in ceramics, and as the raw material for phosphoric acid production.

Eigenschaften

Typ
Precipitation
Reversibel
Nein
Energie
Exotherm
ΔH
-105,0 kJ/mol

Verwandte Reaktionen

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.