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3CaSO3 + 2H3PO4 → Ca3(PO4)2 + 3H2SO3

The reaction of calcium sulfite and phosphoric acid yields calcium phosphate and sulfurous acid (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

General equation

Oxidation state of each atom

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
CaSO3Calcium sulfite3
Brønsted base
Salt of volatile acid
H3PO4Phosphoric acid2
Brønsted acid
Nonvolatile acid

Products

Chemical formulaNameCoefficientTypeType in general
equation
Ca3(PO4)2Calcium phosphate1
Conjugate base
Salt of non volatile acid
H2SO3Sulfurous acid3
Conjugate acid
Volatile acid

Thermodynamic changes

Changes in standard condition (1)

Reaction of calcium sulfite and phosphoric acid
3CaSO3Crystalline solid + 2H3PO4Un-ionized aqueous solution
Ca3(PO4)2Crystalline solidβ, low temp. form + 3H2SO3Un-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
312.1
per 1 mol of
104.0
per 1 mol of
156.1
per 1 mol of
312.1
per 1 mol of
104.0

Changes in standard condition (2)

Reaction of calcium sulfite and phosphoric acid
3CaSO3Crystalline solid + 2H3PO4Un-ionized aqueous solution
Ca3(PO4)2Crystalline solidα, high temp. form + 3H2SO3Un-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
317.0
per 1 mol of
105.7
per 1 mol of
158.5
per 1 mol of
317.0
per 1 mol of
105.7

Changes in standard condition (3)

Reaction of calcium sulfite and phosphoric acid
3CaSO3Crystalline solid + 2H3PO4Ionized aqueous solution
Ca3(PO4)2Crystalline solidβ, low temp. form + 3H2SO3Un-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
1069.1
per 1 mol of
356.37
per 1 mol of
534.55
per 1 mol of
1069.1
per 1 mol of
356.37

Changes in standard condition (4)

Reaction of calcium sulfite and phosphoric acid
3CaSO3Crystalline solid + 2H3PO4Ionized aqueous solution
Ca3(PO4)2Crystalline solidα, high temp. form + 3H2SO3Un-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
1074.0
per 1 mol of
358.00
per 1 mol of
537.00
per 1 mol of
1074.0
per 1 mol of
358.00

Changes in standard condition (5)

Reaction of calcium sulfite and phosphoric acid
3CaSO3Crystalline solid + 2H3PO4Un-ionized aqueous solution
Ca3(PO4)2Crystalline solidβ, low temp. form + 3H2SO3Un-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
312.1
per 1 mol of
104.0
per 1 mol of
156.1
per 1 mol of
312.1
per 1 mol of
104.0

Changes in standard condition (6)

Reaction of calcium sulfite and phosphoric acid
3CaSO3Crystalline solid + 2H3PO4Un-ionized aqueous solution
Ca3(PO4)2Crystalline solidα, high temp. form + 3H2SO3Un-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
317.0
per 1 mol of
105.7
per 1 mol of
158.5
per 1 mol of
317.0
per 1 mol of
105.7

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
CaSO3 (cr)101.38[1]91.71[1]
CaSO3 (cr)
0.5 hydrate
-1311.7[1]-1199.23[1]121.3[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
Ca3(PO4)2 (cr)
β, low temp. form
-4120.8[1]-3884.7[1]236.0[1]227.82[1]
Ca3(PO4)2 (cr)
α, high temp. form
-4109.9[1]-3875.5[1]240.91[1]231.58[1]
Ca3(PO4)2 (ai)-4183.2[1]-3698.1[1]-599.9[1]
H2SO3 (ao)-608.81[1]-537.81[1]232.2[1]
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution

References

List of references

  1. 1