Mn(CH3COO)2 + 2KOH → 2CH3COOK + Mn(OH)2↓
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The reaction of manganese(II) acetate and potassium hydroxide yields potassium acetate and manganese(II) hydroxide. This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of manganese(II) acetate and potassium hydroxide
General equation
- Reaction of salt of weak base and strong base
- Salt of weak baseBrønsted acid + Strong baseBrønsted base ⟶ Salt of strong baseConjugate acid + Weak baseConjugate base + (H2O)
- 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 manganese(II) acetate and potassium hydroxide
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Mn(CH3COO)2 | Manganese(II) acetate | 1 | Brønsted acid Lewis acid | Salt of weak base Very soluble in water |
| KOH | Potassium hydroxide | 2 | Brønsted base Lewis base | Strong base Very soluble in water |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| CH3COOK | Potassium acetate | 2 | Conjugate acid Non-redox product | Salt of strong base – |
| Mn(OH)2 | Manganese(II) hydroxide | 1 | Conjugate base Lewis conjugate | Weak base Insoluble in water |
Thermodynamic changes
Changes in standard condition
- Reaction of manganese(II) acetate and potassium hydroxide
- Mn(CH3COO)2Crystalline solid + 2KOHCrystalline solid2CH3COOKCrystalline solid + Mn(OH)2↓Amorphous solidprecipitated⟶
| 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 | −143.8 | – | – | – |
per 1 mol of | −143.8 | – | – | – |
per 1 mol of | −71.90 | – | – | – |
per 1 mol of | −71.90 | – | – | – |
per 1 mol of | −143.8 | – | – | – |
Changes in aqueous solution
- Reaction of manganese(II) acetate and potassium hydroxide
- Mn(CH3COO)2Aqueous solution + 2KOHIonized aqueous solution2CH3COOKIonized aqueous solution + Mn(OH)2↓Amorphous solidprecipitated⟶
| 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 | −8.3 | – | – | – |
per 1 mol of | −8.3 | – | – | – |
per 1 mol of | −4.2 | – | – | – |
per 1 mol of | −4.2 | – | – | – |
per 1 mol of | −8.3 | – | – | – |
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 |
|---|---|---|---|---|
| Mn(CH3COO)2 (cr) | -1148.1[1] | – | – | – |
| Mn(CH3COO)2 (aq) | -1199.1[1] | – | – | – |
| Mn(CH3COO)2 (cr) 4 hydrate | -2338.0[1] | – | – | – |
| KOH (cr) | -424.764[1] | -379.08[1] | 78.9[1] | 64.9[1] |
| KOH (g) | -231.0[1] | -232.6[1] | 238.3[1] | 49.20[1] |
| KOH (ai) | -482.37[1] | -440.50[1] | 91.6[1] | -126.8[1] |
| KOH (cr) 1 hydrate | -748.9[1] | -645.1[1] | 117.2[1] | – |
| KOH (cr) 2 hydrate | -1051.0[1] | -887.3[1] | 150.6[1] | – |
* (cr):Crystalline solid, (aq):Aqueous solution, (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 |
|---|---|---|---|---|
| CH3COOK (cr) | -723.0[1] | – | – | – |
| CH3COOK (ai) | -738.39[1] | -652.58[1] | 189.1[1] | 15.5[1] |
| Mn(OH)2 (am) precipitated | -695.4[1] | -615.0[1] | 99.2[1] | – |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (am):Amorphous solid
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°, -1148.1 kJ · mol−1
- ^ ΔfH°, -1199.1 kJ · mol−1
- ^ ΔfH°, -2338.0 kJ · mol−1
- ^ ΔfH°, -424.764 kJ · mol−1
- ^ ΔfG°, -379.08 kJ · mol−1
- ^ S°, 78.9 J · K−1 · mol−1
- ^ Cp°, 64.9 J · K−1 · mol−1
- ^ ΔfH°, -231.0 kJ · mol−1
- ^ ΔfG°, -232.6 kJ · mol−1
- ^ S°, 238.3 J · K−1 · mol−1
- ^ Cp°, 49.20 J · K−1 · mol−1
- ^ ΔfH°, -482.37 kJ · mol−1
- ^ ΔfG°, -440.50 kJ · mol−1
- ^ S°, 91.6 J · K−1 · mol−1
- ^ Cp°, -126.8 J · K−1 · mol−1
- ^ ΔfH°, -748.9 kJ · mol−1
- ^ ΔfG°, -645.1 kJ · mol−1
- ^ S°, 117.2 J · K−1 · mol−1
- ^ ΔfH°, -1051.0 kJ · mol−1
- ^ ΔfG°, -887.3 kJ · mol−1
- ^ S°, 150.6 J · K−1 · mol−1
- ^ ΔfH°, -723.0 kJ · mol−1
- ^ ΔfH°, -738.39 kJ · mol−1
- ^ ΔfG°, -652.58 kJ · mol−1
- ^ S°, 189.1 J · K−1 · mol−1
- ^ Cp°, 15.5 J · K−1 · mol−1
- ^ ΔfH°, -695.4 kJ · mol−1
- ^ ΔfG°, -615.0 kJ · mol−1
- ^ S°, 99.2 J · K−1 · mol−1