Pb4(OH)44+ + 4H2O → 4Pb(OH)2 + 4H+
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- Reaction of tetralead(II) tetrahydroxide ion and water
The reaction of tetralead(II) tetrahydroxide ion and water yields lead(II) hydroxide and hydrogen 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 tetralead(II) tetrahydroxide ion and water
General equation
- Cation/AnionBrønsted acid + H2OBrønsted base ⟶ Proton accepting ion/BaseConjugate base + H+Conjugate acid
Oxidation state of each atom
- Reaction of tetralead(II) tetrahydroxide ion and water
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Pb4(OH)44+ | Tetralead(II) tetrahydroxide ion | 1 | Brønsted acid | Cation |
| H2O | Water | 4 | Brønsted base | Water |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Pb(OH)2 | Lead(II) hydroxide | 4 | Conjugate base | Base |
| H+ | Hydrogen ion | 4 | Conjugate acid | Hydrogen ion |
Thermodynamic changes
Changes in standard condition
- Reaction of tetralead(II) tetrahydroxide ion and water◆
ΔrG 76.0 kJ/mol K 0.48 × 10−13 pK 13.31
| 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 | – | 76.0 | – | – |
per 1 mol of Tetralead(II) tetrahydroxide ion | – | 76.0 | – | – |
per 1 mol of | – | 19.0 | – | – |
per 1 mol of | – | 19.0 | – | – |
per 1 mol of Hydrogen ion | – | 19.0 | – | – |
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 |
|---|---|---|---|---|
| Pb4(OH)44+ (ao) | -1066.1[1] | -936.3[1] | 234[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] |
* (ao):Un-ionized aqueous solution, (cr):Crystalline solid, (l):Liquid, (g):Gas
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 |
|---|---|---|---|---|
| Pb(OH)2 (cr) | – | -452.2[1] | – | – |
| Pb(OH)2 (cr) precipitated | -515.9[1] | – | – | – |
| H+ (g) | 1536.202[1] | – | – | – |
| H+ (ao) | 0[1] | 0[1] | 0[1] | 0[1] |
* (cr):Crystalline solid, (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)
- ^ ΔfH°, -1066.1 kJ · mol−1
- ^ ΔfG°, -936.3 kJ · mol−1
- ^ S°, 234. J · K−1 · 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
- ^ ΔfG°, -452.2 kJ · mol−1
- ^ ΔfH°, -515.9 kJ · 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