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2FePO4 + 3Mg(OH)2 → Mg3(PO4)2 + 2Fe(OH)3

The reaction of iron(III) phosphate and magnesium hydroxide yields magnesium phosphate and iron(III) hydroxide. This reaction is an acid-base reaction and is classified as follows:

Table of contents
  1. 1Reaction data
  2. 2Thermodynamic changes
  3. 3References
  4. 4Related categories

Reaction data

Chemical equation

General equation

Oxidation state of each atom

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
FePO4Iron(III) phosphate2
Brønsted acid
Salt of weak base
Mg(OH)2Magnesium hydroxide3
Brønsted base
Strong base

Products

Chemical formulaNameCoefficientTypeType in general
equation
Mg3(PO4)2Magnesium phosphate1
Conjugate acid
Salt of strong base
Fe(OH)3Iron(III) hydroxide2
Conjugate base
Weak base

Thermodynamic changes

Changes in standard condition (1)

Reaction of iron(III) phosphate and magnesium hydroxide
2FePO4Crystalline solid + 3Mg(OH)2Crystalline solid
Mg3(PO4)2Crystalline solid + 2Fe(OH)3Crystalline solidprecipitated
Standard enthalpy
of reaction
ΔrH°
kJ · mol−1
Standard
Gibbs energy
of reaction
ΔrG°
kJ · mol−1
Standard entropy
of reaction
ΔrS°
J · K−1 · mol−1
Standard heat
capacity of reaction
at constant pressure
ΔrCp°
J · K−1 · mol−1
per 1 mol of
Equation
−58.1
−29.1
−19.4
−58.1
−29.1

Changes in standard condition (2)

Reaction of iron(III) phosphate and magnesium hydroxide
2FePO4Crystalline solid + 3Mg(OH)2Amorphous solidprecipitated
Mg3(PO4)2Crystalline solid + 2Fe(OH)3Crystalline solidprecipitated
Standard enthalpy
of reaction
ΔrH°
kJ · mol−1
Standard
Gibbs energy
of reaction
ΔrG°
kJ · mol−1
Standard entropy
of reaction
ΔrS°
J · K−1 · mol−1
Standard heat
capacity of reaction
at constant pressure
ΔrCp°
J · K−1 · mol−1
per 1 mol of
Equation
−70.2
−35.1
−23.4
−70.2
−35.1

Changes in aqueous solution (1)

Reaction of iron(III) phosphate and magnesium hydroxide
2FePO4Crystalline solid + 3Mg(OH)2Crystalline solid
Mg3(PO4)2Crystalline solid + 2Fe(OH)3Un-ionized aqueous solution
Standard enthalpy
of reaction
ΔrH°
kJ · mol−1
Standard
Gibbs energy
of reaction
ΔrG°
kJ · mol−1
Standard entropy
of reaction
ΔrS°
J · K−1 · mol−1
Standard heat
capacity of reaction
at constant pressure
ΔrCp°
J · K−1 · mol−1
per 1 mol of
Equation

Changes in aqueous solution (2)

Reaction of iron(III) phosphate and magnesium hydroxide
2FePO4Crystalline solid + 3Mg(OH)2Amorphous solidprecipitated
Mg3(PO4)2Crystalline solid + 2Fe(OH)3Un-ionized aqueous solution
Standard enthalpy
of reaction
ΔrH°
kJ · mol−1
Standard
Gibbs energy
of reaction
ΔrG°
kJ · mol−1
Standard entropy
of reaction
ΔrS°
J · K−1 · mol−1
Standard heat
capacity of reaction
at constant pressure
ΔrCp°
J · K−1 · mol−1
per 1 mol of
Equation

Thermodynamic data of reactants

Chemical formulaStandard enthalpy
of formation
ΔfH°
kJ · mol−1
Standard Gibbs
energy of
formation
ΔfG°
kJ · mol−1
Standard
molar entropy
S°
J · K−1 · mol−1
Standard molar
heat capacity at
constant pressure
Cp°
J · K−1 · mol−1
FePO4 (cr)-1297.5[1]
FePO4 (cr)
2 hydrate
strengite
-1888.2[1]-1657.5[1]171.25[1]180.54[1]
Mg(OH)2 (cr)-924.54[1]-833.51[1]63.18[1]77.03[1]
Mg(OH)2 (am)
precipitated
-920.5[1]
Mg(OH)2 (g)-561[1]
Mg(OH)2 (ai)-926.84[1]-769.4[1]-159.4[1]
* (cr):Crystalline solid, (am):Amorphous solid, (g):Gas, (ai):Ionized aqueous solution

Thermodynamic data of products

Chemical formulaStandard enthalpy
of formation
ΔfH°
kJ · mol−1
Standard Gibbs
energy of
formation
ΔfG°
kJ · mol−1
Standard
molar entropy
S°
J · K−1 · mol−1
Standard molar
heat capacity at
constant pressure
Cp°
J · K−1 · mol−1
Mg3(PO4)2 (cr)-3780.7[1]-3538.7[1]189.20[1]213.47[1]
Fe(OH)3 (cr)
precipitated
-823.0[1]-696.5[1]106.7[1]
Fe(OH)3 (ao)-659.3[1]
* (cr):Crystalline solid, (ao):Un-ionized aqueous solution

References

List of references

  1. 1