MgSO4 + Na2SO3 💧→ MgSO3↓ + Na2SO4
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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
Reaction data
Chemical equation
- Reaction of magnesium sulfate and sodium sulfite
General equation
- Precipitation reaction
- Miscible with water/Very soluble in water/Soluble in waterLewis acid + Miscible with water/Very soluble in water/Soluble in waterLewis base💧⟶ Insoluble in water/Very slightly soluble in water/Slightly soluble in waterLewis conjugate + Product(Non-redox product)
Oxidation state of each atom
- Reaction of magnesium sulfate and sodium sulfite
Reactants
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
MgSO4 | Magnesium sulfate | 1 | Lewis acid | Very soluble in water |
Na2SO3 | Sodium sulfite | 1 | Lewis base | Very soluble in water |
Products
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
MgSO3 | Magnesium sulfite | 1 | Lewis conjugate | Slightly soluble in water |
Na2SO4 | Sodium sulfate | 1 | Non-redox product | – |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of magnesium sulfate and sodium sulfite◆
ΔrG −10.9 kJ/mol K 8.12 × 101 pK −1.91
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
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◆
ΔrG 17.7 kJ/mol K 0.79 × 10−3 pK 3.10
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 | 94.2 | 17.7 | 256.1 | – |
per 1 mol of | 94.2 | 17.7 | 256.1 | – |
per 1 mol of | 94.2 | 17.7 | 256.1 | – |
per 1 mol of | 94.2 | 17.7 | 256.1 | – |
per 1 mol of | 94.2 | 17.7 | 256.1 | – |
Changes in aqueous solution (2)
- Reaction of magnesium sulfate and sodium sulfite◆
ΔrG 30.4 kJ/mol K 0.47 × 10−5 pK 5.33
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 | 74.1 | 30.4 | 145.2 | – |
per 1 mol of | 74.1 | 30.4 | 145.2 | – |
per 1 mol of | 74.1 | 30.4 | 145.2 | – |
per 1 mol of | 74.1 | 30.4 | 145.2 | – |
per 1 mol of | 74.1 | 30.4 | 145.2 | – |
Thermodynamic data of reactants
Chemical formula | Standard 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 formula | Standard 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
- 1Janiel J. Reed (1989)The NBS Tables of Chemical Thermodynamic Properties: Selected Values for Inorganic and C1 and C2 Organic Substances in SI UnitsNational Institute of Standards and Technology (NIST)
- ^ ΔfH°, -1284.9 kJ · mol−1
- ^ ΔfG°, -1170.6 kJ · mol−1
- ^ S°, 91.6 J · K−1 · mol−1
- ^ Cp°, 96.48 J · K−1 · mol−1
- ^ ΔfH°, -1376.12 kJ · mol−1
- ^ ΔfG°, -1199.5 kJ · mol−1
- ^ S°, -118.0 J · K−1 · mol−1
- ^ ΔfH°, -1356.0 kJ · mol−1
- ^ ΔfG°, -1212.21 kJ · mol−1
- ^ S°, -7.1 J · K−1 · mol−1
- ^ ΔfH°, -1602.1 kJ · mol−1
- ^ ΔfG°, -1428.7 kJ · mol−1
- ^ S°, 126.4 J · K−1 · mol−1
- ^ ΔfH°, -1574.9 kJ · mol−1
- ^ ΔfG°, -1404.9 kJ · mol−1
- ^ S°, 138.1 J · K−1 · mol−1
- ^ ΔfH°, -1896.2 kJ · mol−1
- ^ ΔfH°, -2496.6 kJ · mol−1
- ^ ΔfH°, -3087.0 kJ · mol−1
- ^ ΔfG°, -2631.8 kJ · mol−1
- ^ S°, 348.1 J · K−1 · mol−1
- ^ Cp°, 348.11 J · K−1 · mol−1
- ^ ΔfH°, -3388.71 kJ · mol−1
- ^ ΔfG°, -2871.5 kJ · mol−1
- ^ S°, 372. J · K−1 · mol−1
- ^ ΔfH°, -1100.8 kJ · mol−1
- ^ ΔfG°, -1012.5 kJ · mol−1
- ^ S°, 145.94 J · K−1 · mol−1
- ^ Cp°, 120.25 J · K−1 · mol−1
- ^ ΔfH°, -1115.87 kJ · mol−1
- ^ ΔfG°, -1010.39 kJ · mol−1
- ^ S°, 87.9 J · K−1 · mol−1
- ^ ΔfH°, -3162.3 kJ · mol−1
- ^ ΔfG°, -2676.1 kJ · mol−1
- ^ S°, 444. J · K−1 · mol−1
- ^ ΔfH°, -1008.3 kJ · mol−1
- ^ ΔfG°, -923.8 kJ · mol−1
- ^ S°, 87.9 J · K−1 · mol−1
- ^ ΔfH°, -1931.8 kJ · mol−1
- ^ ΔfG°, -1674.7 kJ · mol−1
- ^ S°, 209.2 J · K−1 · mol−1
- ^ ΔfH°, -2817.5 kJ · mol−1
- ^ ΔfG°, -2385.4 kJ · mol−1
- ^ S°, 322.2 J · K−1 · mol−1
- ^ ΔfH°, -1387.08 kJ · mol−1
- ^ ΔfG°, -1270.16 kJ · mol−1
- ^ S°, 149.58 J · K−1 · mol−1
- ^ Cp°, 128.20 J · K−1 · mol−1
- ^ S°, 154.934 J · K−1 · mol−1
- ^ Cp°, 129.29 J · K−1 · mol−1
- ^ ΔfH°, -1389.51 kJ · mol−1
- ^ ΔfG°, -1268.36 kJ · mol−1
- ^ S°, 138.1 J · K−1 · mol−1
- ^ Cp°, -201. J · K−1 · mol−1
- ^ ΔfH°, -4327.26 kJ · mol−1
- ^ ΔfG°, -3646.85 kJ · mol−1
- ^ S°, 592.0 J · K−1 · mol−1