PbNO3+ + NO3− → Pb(NO3)2
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- Reaction of lead(II) nitrate ion and nitrate ion
The reaction of lead(II) nitrate ion and nitrate ion yields lead(II) nitrate. This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of lead(II) nitrate ion and nitrate ion
General equation
- Reaction of cation and anion
- CationLewis acid + AnionLewis base ⟶ ProductLewis conjugate + (H2O)
Oxidation state of each atom
- Reaction of lead(II) nitrate ion and nitrate ion
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| PbNO3+ | Lead(II) nitrate ion | 1 | Lewis acid | Cation |
| NO3− | Nitrate ion | 1 | Lewis base | Anion |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Pb(NO3)2 | Lead(II) nitrate | 1 | Lewis conjugate | – |
Thermodynamic changes
Changes in standard condition
- Reaction of lead(II) nitrate ion and nitrate ion◆
ΔrG 6.1 kJ/mol K 0.85 × 10−1 pK 1.07 - PbNO3+Un-ionized aqueous solution + NO3−Un-ionized aqueous solutionPb(NO3)2Ionized 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 | – | 6.1 | – | – |
per 1 mol of Lead(II) nitrate ion | – | 6.1 | – | – |
per 1 mol of Nitrate ion | – | 6.1 | – | – |
per 1 mol of | – | 6.1 | – | – |
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 |
|---|---|---|---|---|
| PbNO3+ (ao) | – | -141.8[1] | – | – |
| NO3− (ao) | -207.36[1] | -111.25[1] | 146.4[1] | -86.6[1] |
* (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 |
|---|---|---|---|---|
| Pb(NO3)2 (cr) | -451.9[1] | – | – | – |
| Pb(NO3)2 (ai) | -416.3[1] | -246.93[1] | 303.3[1] | – |
* (cr):Crystalline solid, (ai):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)