Zn(OH)2 → Zn2+ + 2OH−
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- Electrolytic dissociation of zinc hydroxide
Electrolytic dissociation of zinc hydroxide yields zinc ion and 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
- Electrolytic dissociation of zinc hydroxide
General equation
- Electrolytic dissociation of hydroxide base
- Hydroxide baseBrønsted base ⟶ CationConjugate acid + OH−
Oxidation state of each atom
- Electrolytic dissociation of zinc hydroxide
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Zn(OH)2 | Zinc hydroxide | 1 | Brønsted base | Hydroxide base |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Zn2+ | Zinc ion | 1 | Conjugate acid | Cation |
| OH− | Hydroxide ion | 2 | – | Hydroxide ion |
Thermodynamic changes
Changes in standard condition (1)
- Electrolytic dissociation of zinc hydroxide◆
ΔrG 61.18 kJ/mol K 0.19 × 10−10 pK 10.72 - Zn(OH)2Un-ionized aqueous solutionZn2+Un-ionized aqueous solution + 2OH−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 | – | 61.18 | – | – |
per 1 mol of | – | 61.18 | – | – |
per 1 mol of Zinc ion | – | 61.18 | – | – |
per 1 mol of Hydroxide ion | – | 30.59 | – | – |
Changes in standard condition (2)
- Electrolytic dissociation of zinc hydroxide◆
ΔrG 92.26 kJ/mol K 0.69 × 10−16 pK 16.16
| 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 | – | 92.26 | – | – |
per 1 mol of | – | 92.26 | – | – |
per 1 mol of Zinc ion | – | 92.26 | – | – |
per 1 mol of Hydroxide ion | – | 46.13 | – | – |
Changes in standard condition (3)
- Electrolytic dissociation of zinc hydroxide◆
ΔrG 91.97 kJ/mol K 0.77 × 10−16 pK 16.11
| 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 | 28.03 | 91.97 | −214.8 | – |
per 1 mol of | 28.03 | 91.97 | −214.8 | – |
per 1 mol of Zinc ion | 28.03 | 91.97 | −214.8 | – |
per 1 mol of Hydroxide ion | 14.02 | 45.98 | −107.4 | – |
Changes in standard condition (4)
- Electrolytic dissociation of zinc hydroxide◆
ΔrG 93.52 kJ/mol K 0.41 × 10−16 pK 16.38
| 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 | 29.37 | 93.52 | −215.2 | −323 |
per 1 mol of | 29.37 | 93.52 | −215.2 | −323 |
per 1 mol of Zinc ion | 29.37 | 93.52 | −215.2 | −323 |
per 1 mol of Hydroxide ion | 14.69 | 46.76 | −107.6 | −162 |
Changes in standard condition (5)
- Electrolytic dissociation of zinc hydroxide
- Zn(OH)2Crystalline solidprecipitatedZn2+Un-ionized aqueous solution + 2OH−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 | 28.3 | – | – | – |
per 1 mol of | 28.3 | – | – | – |
per 1 mol of Zinc ion | 28.3 | – | – | – |
per 1 mol of Hydroxide ion | 14.2 | – | – | – |
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 |
|---|---|---|---|---|
| Zn(OH)2 (cr) γ | – | -553.81[1] | – | – |
| Zn(OH)2 (cr) β | -641.91[1] | -553.52[1] | 81.2[1] | – |
| Zn(OH)2 (cr) ε | -643.25[1] | -555.07[1] | 81.6[1] | 72.4[1] |
| Zn(OH)2 (cr) precipitated | -642.2[1] | – | – | – |
| Zn(OH)2 (ai) | -613.88[1] | -461.56[1] | -133.5[1] | -251[1] |
| Zn(OH)2 (ao) | – | -522.73[1] | – | – |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (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 |
|---|---|---|---|---|
| Zn2+ (g) | 2782.78[1] | – | – | – |
| Zn2+ (ao) | -153.89[1] | -147.06[1] | -112.1[1] | 46[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
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°, -553.81 kJ · mol−1
- ^ ΔfH°, -641.91 kJ · mol−1
- ^ ΔfG°, -553.52 kJ · mol−1
- ^ S°, 81.2 J · K−1 · mol−1
- ^ ΔfH°, -643.25 kJ · mol−1
- ^ ΔfG°, -555.07 kJ · mol−1
- ^ S°, 81.6 J · K−1 · mol−1
- ^ Cp°, 72.4 J · K−1 · mol−1
- ^ ΔfH°, -642.2 kJ · mol−1
- ^ ΔfH°, -613.88 kJ · mol−1
- ^ ΔfG°, -461.56 kJ · mol−1
- ^ S°, -133.5 J · K−1 · mol−1
- ^ Cp°, -251. J · K−1 · mol−1
- ^ ΔfG°, -522.73 kJ · mol−1
- ^ ΔfH°, 2782.78 kJ · mol−1
- ^ ΔfH°, -153.89 kJ · mol−1
- ^ ΔfG°, -147.06 kJ · mol−1
- ^ S°, -112.1 J · K−1 · mol−1
- ^ Cp°, 46. 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