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  3. 3CaSO3 + 2H3PO4 🔥→ Ca3(PO4)2 + 3SO2↑ + 3H2O

3CaSO3 + 2H3PO4 🔥→ Ca3(PO4)2 + 3SO2↑ + 3H2O

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Reaction of calcium sulfite and phosphoric acid
3CaSO3Calcium sulfite + 2H3PO4Phosphoric acid
🔥
⟶
Ca3(PO4)2Calcium phosphate + 3SO2↑Sulfur dioxide + 3H2OWater

The reaction of calcium sulfite and phosphoric acid yields calcium phosphate, sulfur 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 calcium sulfite and phosphoric acid
3CaSO3Calcium sulfite + 2H3PO4Phosphoric acid
🔥
⟶
Ca3(PO4)2Calcium phosphate + 3SO2↑Sulfur 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 calcium sulfite and phosphoric acid

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
SO2Sulfur dioxide3
–
Volatile acidic oxide
H2OWater3
Conjugate acid
Water

Thermodynamic changes

Changes in standard condition (1)

Reaction of calcium sulfite and phosphoric acid
3CaSO3Crystalline solid + 2H3PO4Crystalline solid
🔥
⟶
Ca3(PO4)2Crystalline solidβ, low temp. form + 3SO2↑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
––665.386.05
per 1 mol of
––221.828.68
per 1 mol of
––332.643.02
per 1 mol of
––665.386.05
per 1 mol of
––221.828.68
per 1 mol of
––221.828.68

Changes in standard condition (2)

Reaction of calcium sulfite and phosphoric acid
3CaSO3Crystalline solid + 2H3PO4Crystalline solid
🔥
⟶
Ca3(PO4)2Crystalline solidα, high temp. form + 3SO2↑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
––670.1689.81
per 1 mol of
––223.3929.94
per 1 mol of
––335.0844.91
per 1 mol of
––670.1689.81
per 1 mol of
––223.3929.94
per 1 mol of
––223.3929.94

Changes in aqueous solution (1)

Reaction of calcium sulfite and phosphoric acid
3CaSO3Crystalline solid + 2H3PO4Un-ionized aqueous solution
🔥
⟶
Ca3(PO4)2Crystalline solidβ, low temp. form + 3SO2↑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
––569.9–
per 1 mol of
––190.0–
per 1 mol of
––284.9–
per 1 mol of
––569.9–
per 1 mol of
––190.0–
per 1 mol of
––190.0–

Changes in aqueous solution (2)

Reaction of calcium sulfite and phosphoric acid
3CaSO3Crystalline solid + 2H3PO4Un-ionized aqueous solution
🔥
⟶
Ca3(PO4)2Crystalline solidβ, low temp. form + 3SO2↑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
––310.9–
per 1 mol of
––103.6–
per 1 mol of
––155.4–
per 1 mol of
––310.9–
per 1 mol of
––103.6–
per 1 mol of
––103.6–

Changes in aqueous solution (3)

Reaction of calcium sulfite and phosphoric acid
3CaSO3Crystalline solid + 2H3PO4Un-ionized aqueous solution
🔥
⟶
Ca3(PO4)2Crystalline solidα, high temp. form + 3SO2↑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
––574.8–
per 1 mol of
––191.6–
per 1 mol of
––287.4–
per 1 mol of
––574.8–
per 1 mol of
––191.6–
per 1 mol of
––191.6–

Changes in aqueous solution (4)

Reaction of calcium sulfite and phosphoric acid
3CaSO3Crystalline solid + 2H3PO4Un-ionized aqueous solution
🔥
⟶
Ca3(PO4)2Crystalline solidα, high temp. form + 3SO2↑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
––315.8–
per 1 mol of
––105.3–
per 1 mol of
––157.9–
per 1 mol of
––315.8–
per 1 mol of
––105.3–
per 1 mol of
––105.3–

Changes in aqueous solution (5)

Reaction of calcium sulfite and phosphoric acid
3CaSO3Crystalline solid + 2H3PO4Ionized aqueous solution
🔥
⟶
Ca3(PO4)2Crystalline solidβ, low temp. form + 3SO2↑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
––1326.9–
per 1 mol of
––442.30–
per 1 mol of
––663.45–
per 1 mol of
––1326.9–
per 1 mol of
––442.30–
per 1 mol of
––442.30–

Changes in aqueous solution (6)

Reaction of calcium sulfite and phosphoric acid
3CaSO3Crystalline solid + 2H3PO4Ionized aqueous solution
🔥
⟶
Ca3(PO4)2Crystalline solidβ, low temp. form + 3SO2↑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
––1067.9–
per 1 mol of
––355.97–
per 1 mol of
––533.95–
per 1 mol of
––1067.9–
per 1 mol of
––355.97–
per 1 mol of
––355.97–

Changes in aqueous solution (7)

Reaction of calcium sulfite and phosphoric acid
3CaSO3Crystalline solid + 2H3PO4Ionized aqueous solution
🔥
⟶
Ca3(PO4)2Crystalline solidα, high temp. form + 3SO2↑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
––1331.8–
per 1 mol of
––443.93–
per 1 mol of
––665.90–
per 1 mol of
––1331.8–
per 1 mol of
––443.93–
per 1 mol of
––443.93–

Changes in aqueous solution (8)

Reaction of calcium sulfite and phosphoric acid
3CaSO3Crystalline solid + 2H3PO4Ionized aqueous solution
🔥
⟶
Ca3(PO4)2Crystalline solidα, high temp. form + 3SO2↑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
––1072.8–
per 1 mol of
––357.60–
per 1 mol of
––536.40–
per 1 mol of
––1072.8–
per 1 mol of
––357.60–
per 1 mol of
––357.60–

Changes in aqueous solution (9)

Reaction of calcium sulfite and phosphoric acid
3CaSO3Crystalline solid + 2H3PO4Un-ionized aqueous solution
🔥
⟶
Ca3(PO4)2Crystalline solidβ, low temp. form + 3SO2↑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
––569.9–
per 1 mol of
––190.0–
per 1 mol of
––284.9–
per 1 mol of
––569.9–
per 1 mol of
––190.0–
per 1 mol of
––190.0–

Changes in aqueous solution (10)

Reaction of calcium sulfite and phosphoric acid
3CaSO3Crystalline solid + 2H3PO4Un-ionized aqueous solution
🔥
⟶
Ca3(PO4)2Crystalline solidβ, low temp. form + 3SO2↑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
––310.9–
per 1 mol of
––103.6–
per 1 mol of
––155.4–
per 1 mol of
––310.9–
per 1 mol of
––103.6–
per 1 mol of
––103.6–

Changes in aqueous solution (11)

Reaction of calcium sulfite and phosphoric acid
3CaSO3Crystalline solid + 2H3PO4Un-ionized aqueous solution
🔥
⟶
Ca3(PO4)2Crystalline solidα, high temp. form + 3SO2↑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
––574.8–
per 1 mol of
––191.6–
per 1 mol of
––287.4–
per 1 mol of
––574.8–
per 1 mol of
––191.6–
per 1 mol of
––191.6–

Changes in aqueous solution (12)

Reaction of calcium sulfite and phosphoric acid
3CaSO3Crystalline solid + 2H3PO4Un-ionized aqueous solution
🔥
⟶
Ca3(PO4)2Crystalline solidα, high temp. form + 3SO2↑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
––315.8–
per 1 mol of
––105.3–
per 1 mol of
––157.9–
per 1 mol of
––315.8–
per 1 mol of
––105.3–
per 1 mol of
––105.3–

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]–
SO2 (l)-320.5[1]–––
SO2 (g)-296.830[1]-300.194[1]248.22[1]39.87[1]
SO2 (ao)-322.980[1]-300.676[1]161.9[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, (ai):Ionized aqueous solution, (l):Liquid, (g):Gas, (ao):Un-ionized aqueous solution

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)