Pb2+ + SO42− → PbSO4↓
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- Reaction of lead(II) ion and sulfate ion
The reaction of lead(II) ion and sulfate ion yields lead(II) sulfate (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) ion and sulfate ion
General equation
- Reaction of cation and anion
- CationLewis acid + AnionLewis base ⟶ ProductLewis conjugate + (H2O)
- Precipitation reaction of cation and anion
- CationLewis acid + AnionLewis base ⟶ Insoluble in water/Very slightly soluble in water/Slightly soluble in waterLewis conjugate + (H2O)
Oxidation state of each atom
- Reaction of lead(II) ion and sulfate ion
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Pb2+ | Lead(II) ion | 1 | Lewis acid | Cation |
| SO42− | Sulfate ion | 1 | Lewis base | Anion |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| PbSO4 | Lead(II) sulfate | 1 | Lewis conjugate | – Insoluble in water |
Thermodynamic changes
Changes in standard condition
- Reaction of lead(II) ion and sulfate ion◆
ΔrG −44.18 kJ/mol K 5.50 × 107 pK −7.74
| 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 | −9.0 | −44.18 | 118.0 | – |
per 1 mol of Lead(II) ion | −9.0 | −44.18 | 118.0 | – |
per 1 mol of Sulfate ion | −9.0 | −44.18 | 118.0 | – |
per 1 mol of | −9.0 | −44.18 | 118.0 | – |
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 |
|---|---|---|---|---|
| Pb2+ (g) | 2373.33[1] | – | – | – |
| Pb2+ (ao) | -1.7[1] | -24.43[1] | 10.5[1] | – |
| SO42− (ao) | -909.27[1] | -744.53[1] | 20.1[1] | -293[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 |
|---|---|---|---|---|
| PbSO4 (cr) | -919.94[1] | -813.14[1] | 148.57[1] | 103.207[1] |
* (cr):Crystalline solid
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°, 2373.33 kJ · mol−1
- ^ ΔfH°, -1.7 kJ · mol−1
- ^ ΔfG°, -24.43 kJ · mol−1
- ^ S°, 10.5 J · K−1 · mol−1
- ^ ΔfH°, -909.27 kJ · mol−1
- ^ ΔfG°, -744.53 kJ · mol−1
- ^ S°, 20.1 J · K−1 · mol−1
- ^ Cp°, -293. J · K−1 · mol−1
- ^ ΔfH°, -919.94 kJ · mol−1
- ^ ΔfG°, -813.14 kJ · mol−1
- ^ S°, 148.57 J · K−1 · mol−1
- ^ Cp°, 103.207 J · K−1 · mol−1