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  3. 3MgCO3 + 2H3PO4 🔥→ Mg3(PO4)2 + 3CO2↑ + 3H2O

3MgCO3 + 2H3PO4 🔥→ Mg3(PO4)2 + 3CO2↑ + 3H2O

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Reaction of magnesium carbonate and phosphoric acid
3MgCO3Magnesium carbonate + 2H3PO4Phosphoric acid
🔥
⟶
Mg3(PO4)2Magnesium phosphate + 3CO2↑Carbon dioxide + 3H2OWater

The reaction of magnesium carbonate and phosphoric acid yields magnesium phosphate, carbon dioxide, and water (Other reactions are here). 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 reactions
  5. 5Related categories

Reaction data

Chemical equation

Reaction of magnesium carbonate and phosphoric acid
3MgCO3Magnesium carbonate + 2H3PO4Phosphoric acid
🔥
⟶
Mg3(PO4)2Magnesium phosphate + 3CO2↑Carbon dioxide + 3H2OWater

General equation

Reaction of salt of volatile acid and nonvolatile acid with generating volatile acidic oxide
Salt of volatile acidBrønsted base + Nonvolatile acidBrønsted acid
⟶
Salt of non volatile acidConjugate base + Volatile acidic oxide + H2OConjugate acid

Oxidation state of each atom

Reaction of magnesium carbonate and phosphoric acid

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
MgCO3Magnesium carbonate3
Brønsted base
Salt of volatile acid
H3PO4Phosphoric acid2
Brønsted acid
Nonvolatile acid

Products

Chemical formulaNameCoefficientTypeType in general
equation
Mg3(PO4)2Magnesium phosphate1
Conjugate base
Salt of non volatile acid
CO2Carbon dioxide3
–
Volatile acidic oxide
H2OWater3
Conjugate acid
Water

Thermodynamic changes

Changes in standard condition

Reaction of magnesium carbonate and phosphoric acid
◆
ΔrG−158.7 kJ/mol
K6.35 × 1027
pK−27.80
3MgCO3Crystalline solid + 2H3PO4Crystalline solid
🔥
⟶
Mg3(PO4)2Crystalline solid + 3CO2↑Gas + 3H2OLiquid
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
26.7−158.7622.1111.99
8.90−52.90207.437.330
per 1 mol of
13.3−79.35311.155.995
26.7−158.7622.1111.99
per 1 mol of
8.90−52.90207.437.330
per 1 mol of
8.90−52.90207.437.330

Changes in aqueous solution (1)

Reaction of magnesium carbonate and phosphoric acid
◆
ΔrG−111.8 kJ/mol
K3.86 × 1019
pK−19.59
3MgCO3Crystalline solid + 2H3PO4Un-ionized aqueous solution
🔥
⟶
Mg3(PO4)2Crystalline solid + 3CO2↑Gas + 3H2OLiquid
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
45.4−111.8526.7–
15.1−37.27175.6–
per 1 mol of
22.7−55.90263.4–
45.4−111.8526.7–
per 1 mol of
15.1−37.27175.6–
per 1 mol of
15.1−37.27175.6–

Changes in aqueous solution (2)

Reaction of magnesium carbonate and phosphoric acid
◆
ΔrG−86.6 kJ/mol
K1.48 × 1015
pK−15.17
3MgCO3Crystalline solid + 2H3PO4Un-ionized aqueous solution
🔥
⟶
Mg3(PO4)2Crystalline solid + 3CO2↑Un-ionized aqueous solution + 3H2OLiquid
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
−15.5−86.6238.2–
−5.17−28.979.40–
per 1 mol of
−7.75−43.3119.1–
−15.5−86.6238.2–
per 1 mol of
−5.17−28.979.40–
per 1 mol of
−5.17−28.979.40–

Changes in aqueous solution (3)

Reaction of magnesium carbonate and phosphoric acid
◆
ΔrG−359.5 kJ/mol
K9.59 × 1062
pK−62.98
3MgCO3Crystalline solid + 2H3PO4Ionized aqueous solution
🔥
⟶
Mg3(PO4)2Crystalline solid + 3CO2↑Gas + 3H2OLiquid
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
23.5−359.51283.7–
7.83−119.8427.90–
per 1 mol of
11.8−179.8641.85–
23.5−359.51283.7–
per 1 mol of
7.83−119.8427.90–
per 1 mol of
7.83−119.8427.90–

Changes in aqueous solution (4)

Reaction of magnesium carbonate and phosphoric acid
◆
ΔrG−334.3 kJ/mol
K3.69 × 1058
pK−58.57
3MgCO3Crystalline solid + 2H3PO4Ionized aqueous solution
🔥
⟶
Mg3(PO4)2Crystalline solid + 3CO2↑Un-ionized aqueous solution + 3H2OLiquid
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
−37.4−334.3995.2–
−12.5−111.4331.7–
per 1 mol of
−18.7−167.2497.6–
−37.4−334.3995.2–
per 1 mol of
−12.5−111.4331.7–
per 1 mol of
−12.5−111.4331.7–

Changes in aqueous solution (5)

Reaction of magnesium carbonate and phosphoric acid
◆
ΔrG−111.8 kJ/mol
K3.86 × 1019
pK−19.59
3MgCO3Crystalline solid + 2H3PO4Un-ionized aqueous solution
🔥
⟶
Mg3(PO4)2Crystalline solid + 3CO2↑Gas + 3H2OLiquid
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
45.4−111.8526.7–
15.1−37.27175.6–
per 1 mol of
22.7−55.90263.4–
45.4−111.8526.7–
per 1 mol of
15.1−37.27175.6–
per 1 mol of
15.1−37.27175.6–

Changes in aqueous solution (6)

Reaction of magnesium carbonate and phosphoric acid
◆
ΔrG−86.6 kJ/mol
K1.48 × 1015
pK−15.17
3MgCO3Crystalline solid + 2H3PO4Un-ionized aqueous solution
🔥
⟶
Mg3(PO4)2Crystalline solid + 3CO2↑Un-ionized aqueous solution + 3H2OLiquid
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
−15.5−86.6238.2–
−5.17−28.979.40–
per 1 mol of
−7.75−43.3119.1–
−15.5−86.6238.2–
per 1 mol of
−5.17−28.979.40–
per 1 mol of
−5.17−28.979.40–

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
MgCO3 (cr)-1095.8[1]-1012.1[1]65.7[1]75.52[1]
MgCO3 (cr)
3 hydrate
–-1726.1[1]––
MgCO3 (cr)
5 hydrate
–-2199.2[1]––
H3PO4 (cr)-1279.0[1]-1119.1[1]110.50[1]106.06[1]
H3PO4 (l)-1266.9[1]–––
H3PO4 (ai)-1277.4[1]-1018.7[1]-220.3[1]–
H3PO4 (ao)-1288.34[1]-1142.54[1]158.2[1]–
H3PO4 (cr)
0.5 hydrate
-1431.3[1]-1242.1[1]129.16[1]126.02[1]
H3PO4 (cr)
1 hydrate
-1568.83[1]–––
* (cr):Crystalline solid, (l):Liquid, (ai):Ionized aqueous solution, (ao):Un-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]
CO2 (g)-393.509[1]-394.359[1]213.74[1]37.11[1]
CO2 (ao)-413.80[1]-385.98[1]117.6[1]–
H2O (cr)––––
H2O (l)-285.830[1]-237.129[1]69.91[1]75.291[1]
H2O (g)-241.818[1]-228.572[1]188.825[1]33.577[1]
* (cr):Crystalline solid, (g):Gas, (ao):Un-ionized aqueous solution, (l):Liquid

References

List of references

  1. 1
    Janiel J. Reed (1989)
    The NBS Tables of Chemical Thermodynamic Properties: Selected Values for Inorganic and C1 and C2 Organic Substances in SI Units
    National Institute of Standards and Technology (NIST)