2Pb(OH)2 + Pb4(OH)44+ → 2Pb3(OH)42+
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- Reaction of lead(II) hydroxide and tetralead(II) tetrahydroxide ion
- 2Pb(OH)2Lead(II) hydroxide + Pb4(OH)44+Tetralead(II) tetrahydroxide ion2Pb3(OH)42+Trilead(II) tetrahydroxide ion⟶
The reaction of lead(II) hydroxide and tetralead(II) tetrahydroxide ion yields trilead(II) tetrahydroxide 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 lead(II) hydroxide and tetralead(II) tetrahydroxide ion
- 2Pb(OH)2Lead(II) hydroxide + Pb4(OH)44+Tetralead(II) tetrahydroxide ion2Pb3(OH)42+Trilead(II) tetrahydroxide ion⟶
General equation
- Reaction of neutral species and cation
- CompoundLewis base + CationLewis acid ⟶ CationLewis conjugate
Oxidation state of each atom
- Reaction of lead(II) hydroxide and tetralead(II) tetrahydroxide ion
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Pb(OH)2 | Lead(II) hydroxide | 2 | Lewis base | Compound |
| Pb4(OH)44+ | Tetralead(II) tetrahydroxide ion | 1 | Lewis acid | Cation |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Pb3(OH)42+ | Trilead(II) tetrahydroxide ion | 2 | Lewis conjugate | Cation |
Thermodynamic changes
Changes in standard condition
- Reaction of lead(II) hydroxide and tetralead(II) tetrahydroxide ion◆
ΔrG 63.5 kJ/mol K 0.75 × 10−11 pK 11.12 - 2Pb(OH)2Crystalline solid + Pb4(OH)44+Un-ionized aqueous solution2Pb3(OH)42+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 | – | 63.5 | – | – |
per 1 mol of | – | 31.8 | – | – |
per 1 mol of Tetralead(II) tetrahydroxide ion | – | 63.5 | – | – |
per 1 mol of Trilead(II) tetrahydroxide ion | – | 31.8 | – | – |
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 |
|---|---|---|---|---|
| Pb(OH)2 (cr) | – | -452.2[1] | – | – |
| Pb(OH)2 (cr) precipitated | -515.9[1] | – | – | – |
| Pb4(OH)44+ (ao) | -1066.1[1] | -936.3[1] | 234[1] | – |
* (cr):Crystalline solid, (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 |
|---|---|---|---|---|
| Pb3(OH)42+ (ao) | -1037.6[1] | -888.6[1] | 234[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)