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MgSO4 + Na2SO3 💧→ MgSO3↓ + Na2SO4

The reaction of magnesium sulfate and sodium sulfite yields magnesium sulfite and sodium sulfate. 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
MgSO4Magnesium sulfate1
Lewis acid
Very soluble in water
Na2SO3Sodium sulfite1
Lewis base
Very soluble in water

Products

Chemical formulaNameCoefficientTypeType in general
equation
MgSO3Magnesium sulfite1
Lewis conjugate
Slightly soluble in water
Na2SO4Sodium sulfate1
Non-redox product

Thermodynamic changes

Changes in standard condition (1)

Reaction of magnesium sulfate and sodium sulfite
ΔrG−10.9 kJ/mol
K8.12 × 101
pK−1.91
MgSO4Crystalline solid + Na2SO3Crystalline solid
💧
MgSO3Crystalline solid + Na2SO4Crystalline solidorthorhombic
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
−9.7−10.9−0.1
per 1 mol of
−9.7−10.9−0.10
per 1 mol of
−9.7−10.9−0.10
per 1 mol of
−9.7−10.9−0.10
per 1 mol of
−9.7−10.9−0.10

Changes in standard condition (2)

Reaction of magnesium sulfate and sodium sulfite
MgSO4Crystalline solid + Na2SO3Crystalline solid
💧
MgSO3Crystalline solid + Na2SO4Crystalline solidmetastable
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
5.3
per 1 mol of
5.3
per 1 mol of
5.3
per 1 mol of
5.3
per 1 mol of
5.3

Changes in aqueous solution (1)

Reaction of magnesium sulfate and sodium sulfite
ΔrG17.7 kJ/mol
K0.79 × 10−3
pK3.10
MgSO4Ionized aqueous solution + Na2SO3Ionized aqueous solution
💧
MgSO3Crystalline solid + Na2SO4Ionized 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
94.217.7256.1
per 1 mol of
94.217.7256.1
per 1 mol of
94.217.7256.1
per 1 mol of
94.217.7256.1
per 1 mol of
94.217.7256.1

Changes in aqueous solution (2)

Reaction of magnesium sulfate and sodium sulfite
ΔrG30.4 kJ/mol
K0.47 × 10−5
pK5.33
MgSO4Un-ionized aqueous solution + Na2SO3Ionized aqueous solution
💧
MgSO3Crystalline solid + Na2SO4Ionized 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
74.130.4145.2
per 1 mol of
74.130.4145.2
per 1 mol of
74.130.4145.2
per 1 mol of
74.130.4145.2
per 1 mol of
74.130.4145.2

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
MgSO4 (cr)-1284.9[1]-1170.6[1]91.6[1]96.48[1]
MgSO4 (ai)-1376.12[1]-1199.5[1]-118.0[1]
MgSO4 (ao)-1356.0[1]-1212.21[1]-7.1[1]
MgSO4 (cr)
1 hydrate
-1602.1[1]-1428.7[1]126.4[1]
MgSO4 (am)
1 hydrate
-1574.9[1]-1404.9[1]138.1[1]
MgSO4 (cr)
2 hydrate
-1896.2[1]
MgSO4 (cr)
4 hydrate
-2496.6[1]
MgSO4 (cr)
6 hydrate
-3087.0[1]-2631.8[1]348.1[1]348.11[1]
MgSO4 (cr)
7 hydrate
-3388.71[1]-2871.5[1]372[1]
Na2SO3 (cr)-1100.8[1]-1012.5[1]145.94[1]120.25[1]
Na2SO3 (ai)-1115.87[1]-1010.39[1]87.9[1]
Na2SO3 (cr)
7 hydrate
-3162.3[1]-2676.1[1]444[1]
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution, (am):Amorphous solid

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
MgSO3 (cr)-1008.3[1]-923.8[1]87.9[1]
MgSO3 (cr)
3 hydrate
-1931.8[1]-1674.7[1]209.2[1]
MgSO3 (cr)
6 hydrate
-2817.5[1]-2385.4[1]322.2[1]
Na2SO4 (cr)
orthorhombic
-1387.08[1]-1270.16[1]149.58[1]128.20[1]
Na2SO4 (cr)
metastable
154.934[1]129.29[1]
Na2SO4 (ai)-1389.51[1]-1268.36[1]138.1[1]-201[1]
Na2SO4 (cr)
10 hydrate
-4327.26[1]-3646.85[1]592.0[1]
* (cr):Crystalline solid, (ai):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)