MgHCO3+ → Mg2+ + H+ + CO32−
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- Electrolytic dissociation of magnesium hydrogencarbonate ion
- MgHCO3+Magnesium hydrogencarbonate ionMg2+Magnesium ion + H+Hydrogen ion + CO32−Carbonate ion⟶
Electrolytic dissociation of magnesium hydrogencarbonate ion yields magnesium ion, hydrogen ion, and carbonate ion (Other reactions are here). This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Electrolytic dissociation of magnesium hydrogencarbonate ion
- MgHCO3+Magnesium hydrogencarbonate ionMg2+Magnesium ion + H+Hydrogen ion + CO32−Carbonate ion⟶
General equation
- Electrolytic dissociation of ion
- Polyatomic ion ⟶ Cation/Electrically neutral + Anion/Electrically neutral
- Electrolytic dissociation of proton donating ion
- Proton donating ionBrønsted acid ⟶ H+ + Proton accepting/Proton accepting ionConjugate base
Oxidation state of each atom
- Electrolytic dissociation of magnesium hydrogencarbonate ion
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| MgHCO3+ | Magnesium hydrogencarbonate ion | 1 | – Brønsted acid | Polyatomic ion Proton donating ion |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Mg2+ | Magnesium ion | 1 | – | Cation |
| H+ | Hydrogen ion | 1 | – | Cation |
| CO32− | Carbonate ion | 1 | – | Anion |
Thermodynamic changes
Changes in standard condition
- Electrolytic dissociation of magnesium hydrogencarbonate ion◆
ΔrG 64.6 kJ/mol K 0.48 × 10−11 pK 11.32 - MgHCO3+Un-ionized aqueous solutionMg2+Un-ionized aqueous solution + H+Un-ionized aqueous solution + CO32−Un-ionized 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 | – | 64.6 | – | – |
per 1 mol of Magnesium hydrogencarbonate ion | – | 64.6 | – | – |
per 1 mol of Magnesium ion | – | 64.6 | – | – |
per 1 mol of Hydrogen ion | – | 64.6 | – | – |
per 1 mol of Carbonate ion | – | 64.6 | – | – |
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 |
|---|---|---|---|---|
| MgHCO3+ (ao) | – | -1047.2[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 |
|---|---|---|---|---|
| Mg2+ (g) | 2348.504[1] | – | – | – |
| Mg2+ (ao) | -466.85[1] | -454.8[1] | -138.1[1] | – |
| H+ (g) | 1536.202[1] | – | – | – |
| H+ (ao) | 0[1] | 0[1] | 0[1] | 0[1] |
| CO32− (ao) | -677.14[1] | -527.81[1] | -56.9[1] | – |
* (g):Gas, (ao):Un-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)
- ^ ΔfG°, -1047.2 kJ · mol−1
- ^ ΔfH°, 2348.504 kJ · mol−1
- ^ ΔfH°, -466.85 kJ · mol−1
- ^ ΔfG°, -454.8 kJ · mol−1
- ^ S°, -138.1 J · K−1 · mol−1
- ^ ΔfH°, 1536.202 kJ · mol−1
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 0 J · K−1 · mol−1
- ^ Cp°, 0 J · K−1 · mol−1
- ^ ΔfH°, -677.14 kJ · mol−1
- ^ ΔfG°, -527.81 kJ · mol−1
- ^ S°, -56.9 J · K−1 · mol−1