H2SO3 + Mg(OH)2 → MgSO3 + 2H2O
Last updated:
The reaction of sulfurous acid and magnesium hydroxide yields magnesium sulfite and water. This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of sulfurous acid and magnesium hydroxide
General equation
- Reaction of acid and base
- AcidBrønsted acid + BaseBrønsted base ⟶ SaltConjugate base + (H2O)(Conjugate acid)
- Reaction of acid and hydroxide base
- AcidBrønsted acid + Hydroxide baseBrønsted base ⟶ SaltConjugate base + H2OConjugate acid
- Reaction of weak acid and strong base
- Weak acidBrønsted acid + Strong baseBrønsted base ⟶ Salt of weak acid and strong baseConjugate base + (H2O)(Conjugate acid)
Oxidation state of each atom
- Reaction of sulfurous acid and magnesium hydroxide
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| H2SO3 | Sulfurous acid | 1 | Brønsted acid | Acid Weak acid |
| Mg(OH)2 | Magnesium hydroxide | 1 | Brønsted base | Base Hydroxide base Strong base |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| MgSO3 | Magnesium sulfite | 1 | Conjugate base | Salt Salt of weak acid and strong base |
| H2O | Water | 2 | Conjugate acid | Water |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of sulfurous acid and magnesium hydroxide◆
ΔrG −26.7 kJ/mol K 4.76 × 104 pK −4.68
| 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 | −46.6 | −26.7 | −67.7 | – |
per 1 mol of | −46.6 | −26.7 | −67.7 | – |
per 1 mol of | −46.6 | −26.7 | −67.7 | – |
per 1 mol of | −46.6 | −26.7 | −67.7 | – |
per 1 mol of | −23.3 | −13.3 | −33.9 | – |
Changes in standard condition (2)
- Reaction of sulfurous acid and magnesium hydroxide
| 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 | −50.7 | – | – | – |
per 1 mol of | −50.7 | – | – | – |
per 1 mol of | −50.7 | – | – | – |
per 1 mol of | −50.7 | – | – | – |
per 1 mol of | −25.4 | – | – | – |
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 |
|---|---|---|---|---|
| H2SO3 (ao) | -608.81[1] | -537.81[1] | 232.2[1] | – |
| Mg(OH)2 (cr) | -924.54[1] | -833.51[1] | 63.18[1] | 77.03[1] |
| Mg(OH)2 (am) precipitated | -920.5[1] | – | – | – |
| Mg(OH)2 (g) | -561[1] | – | – | – |
| Mg(OH)2 (ai) | -926.84[1] | -769.4[1] | -159.4[1] | – |
* (ao):Un-ionized aqueous solution, (cr):Crystalline solid, (am):Amorphous solid, (g):Gas, (ai):Ionized aqueous solution
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] | – |
| 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, (l):Liquid, (g):Gas
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°, -608.81 kJ · mol−1
- ^ ΔfG°, -537.81 kJ · mol−1
- ^ S°, 232.2 J · K−1 · mol−1
- ^ ΔfH°, -924.54 kJ · mol−1
- ^ ΔfG°, -833.51 kJ · mol−1
- ^ S°, 63.18 J · K−1 · mol−1
- ^ Cp°, 77.03 J · K−1 · mol−1
- ^ ΔfH°, -920.5 kJ · mol−1
- ^ ΔfH°, -561. kJ · mol−1
- ^ ΔfH°, -926.84 kJ · mol−1
- ^ ΔfG°, -769.4 kJ · mol−1
- ^ S°, -159.4 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°, -285.830 kJ · mol−1
- ^ ΔfG°, -237.129 kJ · mol−1
- ^ S°, 69.91 J · K−1 · mol−1
- ^ Cp°, 75.291 J · K−1 · mol−1
- ^ ΔfH°, -241.818 kJ · mol−1
- ^ ΔfG°, -228.572 kJ · mol−1
- ^ S°, 188.825 J · K−1 · mol−1
- ^ Cp°, 33.577 J · K−1 · mol−1