MnOH+ + HCO3− → MnCO3↓ + H2O
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- Reaction of manganese(II) hydroxide ion and hydrogencarbonate ion
- MnOH+Manganese(II) hydroxide ion + HCO3−Hydrogencarbonate ionMnCO3↓Manganese(II) carbonate + H2OWater⟶
The reaction of manganese(II) hydroxide ion and hydrogencarbonate ion yields manganese(II) carbonate and water. This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of manganese(II) hydroxide ion and hydrogencarbonate ion
- MnOH+Manganese(II) hydroxide ion + HCO3−Hydrogencarbonate ionMnCO3↓Manganese(II) carbonate + H2OWater⟶
General equation
- Reaction of cation and anion
- CationLewis acid + AnionLewis base ⟶ ProductLewis conjugate + (H2O)
- Precipitation reaction of cation and anion
- CationLewis acid + AnionLewis base ⟶ Insoluble in water/Very slightly soluble in water/Slightly soluble in waterLewis conjugate + (H2O)
Oxidation state of each atom
- Reaction of manganese(II) hydroxide ion and hydrogencarbonate ion
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| MnOH+ | Manganese(II) hydroxide ion | 1 | Lewis acid | Cation |
| HCO3− | Hydrogencarbonate ion | 1 | Lewis base | Anion |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| MnCO3 | Manganese(II) carbonate | 1 | Lewis conjugate | – Insoluble in water |
| H2O | Water | 1 | – | Water |
Thermodynamic changes
Changes in standard condition
- Reaction of manganese(II) hydroxide ion and hydrogencarbonate ion◆
ΔrG −62.1 kJ/mol K 7.58 × 1010 pK −10.88
| 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 | −37.3 | −62.1 | 82 | – |
per 1 mol of Manganese(II) hydroxide ion | −37.3 | −62.1 | 82 | – |
per 1 mol of Hydrogencarbonate ion | −37.3 | −62.1 | 82 | – |
per 1 mol of | −37.3 | −62.1 | 82 | – |
per 1 mol of | −37.3 | −62.1 | 82 | – |
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 |
|---|---|---|---|---|
| MnOH+ (ao) | -450.6[1] | -405.0[1] | -17[1] | – |
| HCO3− (ao) | -691.99[1] | -586.77[1] | 91.2[1] | – |
* (ao):Un-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 |
|---|---|---|---|---|
| MnCO3 (cr) natural | -894.1[1] | -816.7[1] | 85.8[1] | 81.50[1] |
| MnCO3 (cr) precipitated | -883.2[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°, -450.6 kJ · mol−1
- ^ ΔfG°, -405.0 kJ · mol−1
- ^ S°, -17. J · K−1 · mol−1
- ^ ΔfH°, -691.99 kJ · mol−1
- ^ ΔfG°, -586.77 kJ · mol−1
- ^ S°, 91.2 J · K−1 · mol−1
- ^ ΔfH°, -894.1 kJ · mol−1
- ^ ΔfG°, -816.7 kJ · mol−1
- ^ S°, 85.8 J · K−1 · mol−1
- ^ Cp°, 81.50 J · K−1 · mol−1
- ^ ΔfH°, -883.2 kJ · 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