Hg2+ + OH− → HgOH+
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- Reaction of mercury(II) ion and hydroxide ion
- Hg2+Mercury(II) ion + OH−Hydroxide ionHgOH+Mercury(II) hydroxide ion⟶
The reaction of mercury(II) ion and hydroxide ion yields mercury(II) hydroxide ion (Other reactions are here). This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of mercury(II) ion and hydroxide ion
- Hg2+Mercury(II) ion + OH−Hydroxide ionHgOH+Mercury(II) hydroxide ion⟶
General equation
- Reaction of cation and anion
- CationLewis acid + AnionLewis base ⟶ ProductLewis conjugate + (H2O)
- Reaction of cation and hydroxide ion
- CationLewis acid + OH−Lewis base ⟶ Base/Basic salt ionLewis conjugate + (H2O)
Oxidation state of each atom
- Reaction of mercury(II) ion and hydroxide ion
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Hg2+ | Mercury(II) ion | 1 | Lewis acid | Cation |
| OH− | Hydroxide ion | 1 | Lewis base | Anion Hydroxide ion |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| HgOH+ | Mercury(II) hydroxide ion | 1 | Lewis conjugate | – Basic salt ion |
Thermodynamic changes
Changes in standard condition
- Reaction of mercury(II) ion and hydroxide ion◆
ΔrG −59.5 kJ/mol K 2.65 × 1010 pK −10.42 - Hg2+Un-ionized aqueous solution + OH−Un-ionized aqueous solutionHgOH+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 | −25.6 | −59.5 | 114 | – |
per 1 mol of Mercury(II) ion | −25.6 | −59.5 | 114 | – |
per 1 mol of Hydroxide ion | −25.6 | −59.5 | 114 | – |
per 1 mol of Mercury(II) hydroxide ion | −25.6 | −59.5 | 114 | – |
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 |
|---|---|---|---|---|
| Hg2+ (g) | 2890.47[1] | – | – | – |
| Hg2+ (ao) | 171.1[1] | 164.40[1] | -32.2[1] | – |
| OH− (g) | -143.5[1] | – | – | – |
| OH− (ao) | -229.994[1] | -157.244[1] | -10.75[1] | -148.5[1] |
* (g):Gas, (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 |
|---|---|---|---|---|
| HgOH+ (ao) | -84.5[1] | -52.3[1] | 71[1] | – |
* (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)
- ^ ΔfH°, 2890.47 kJ · mol−1
- ^ ΔfH°, 171.1 kJ · mol−1
- ^ ΔfG°, 164.40 kJ · mol−1
- ^ S°, -32.2 J · K−1 · mol−1
- ^ ΔfH°, -143.5 kJ · mol−1
- ^ ΔfH°, -229.994 kJ · mol−1
- ^ ΔfG°, -157.244 kJ · mol−1
- ^ S°, -10.75 J · K−1 · mol−1
- ^ Cp°, -148.5 J · K−1 · mol−1
- ^ ΔfH°, -84.5 kJ · mol−1
- ^ ΔfG°, -52.3 kJ · mol−1
- ^ S°, 71. J · K−1 · mol−1