Calcium Phosphate Precipitation (Bone Mineral)

3CaCl₂ + 2Na₃PO₄ → Ca₃(PO₄)₂↓ + 6NaCl

نظرة عامة

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.

المشاركون

الدور	المادة	المعامل	الحالة
منتج	Sodium Chloride NaCl	6	(aq)

مثال من الحياة اليومية

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

الأهمية الصناعية

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.

الخصائص

النوع: Precipitation
قابل للعكس: لا
الطاقة: طارد للحرارة
ΔH: -105,0 kJ/mol

التفاعلات ذات الصلة

Aluminum Hydroxide Precipitation Barium Sulfate Precipitation Cadmium Sulfide Precipitation (Yellow) Chromium(III) Hydroxide Precipitation Lead Carbonate Precipitation Magnesium Hydroxide Precipitation Copper Sulfide Precipitation Cobalt(II) Hydroxide Precipitation Mercury(II) Sulfide Precipitation (Vermilion) 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.