Pb(CH3COO)2 + 2H2O → Pb(OH)2 + 2CH3COOH
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The reaction of lead(II) acetate and water yields lead(II) hydroxide and acetic acid (Other reactions are here). This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Hydrolysis of lead(II) acetate
General equation
- Hydrolysis of salt
- Salt of weak acid and weak baseBrønsted base + H2OBrønsted acid ⟶ Base/Basic saltConjugate base + Acid/Acid salt/HydrideConjugate acid
Oxidation state of each atom
- Hydrolysis of lead(II) acetate
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Pb(CH3COO)2 | Lead(II) acetate | 1 | Brønsted base | Salt of weak acid and weak base |
| H2O | Water | 2 | Brønsted acid | Water |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Pb(OH)2 | Lead(II) hydroxide | 1 | Conjugate base | Base |
| CH3COOH | Acetic acid | 2 | Conjugate acid | Acid |
Thermodynamic changes
Changes in standard condition (1)
- Hydrolysis of lead(II) acetate
| 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 | – | – | – | – |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
Changes in standard condition (2)
- Hydrolysis of lead(II) acetate
| 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 | 50.6 | – | – | – |
per 1 mol of | 50.6 | – | – | – |
per 1 mol of | 25.3 | – | – | – |
per 1 mol of | 50.6 | – | – | – |
per 1 mol of | 25.3 | – | – | – |
Changes in aqueous solution (1)
- Hydrolysis of lead(II) acetate◆
ΔrG −7.8 kJ/mol K 2.33 × 101 pK −1.37 - Pb(CH3COO)2Ionized aqueous solution + 2H2OLiquidPb(OH)2Crystalline solid + 2CH3COOHUn-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 | – | −7.8 | – | – |
per 1 mol of | – | −7.8 | – | – |
per 1 mol of | – | −3.9 | – | – |
per 1 mol of | – | −7.8 | – | – |
per 1 mol of | – | −3.9 | – | – |
Changes in aqueous solution (2)
- Hydrolysis of lead(II) acetate◆
ΔrG 8.8 kJ/mol K 0.29 × 10−1 pK 1.54 - Pb(CH3COO)2Un-ionized aqueous solution + 2H2OLiquidPb(OH)2Crystalline solid + 2CH3COOHUn-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 | – | 8.8 | – | – |
per 1 mol of | – | 8.8 | – | – |
per 1 mol of | – | 4.4 | – | – |
per 1 mol of | – | 8.8 | – | – |
per 1 mol of | – | 4.4 | – | – |
Changes in aqueous solution (3)
- Hydrolysis of lead(II) acetate◆
ΔrG 46.5 kJ/mol K 0.71 × 10−8 pK 8.15 - Pb(CH3COO)2Ionized aqueous solution + 2H2OLiquidPb(OH)2Crystalline solid + 2CH3COOHIonized 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 | – | 46.5 | – | – |
per 1 mol of | – | 46.5 | – | – |
per 1 mol of | – | 23.3 | – | – |
per 1 mol of | – | 46.5 | – | – |
per 1 mol of | – | 23.3 | – | – |
Changes in aqueous solution (4)
- Hydrolysis of lead(II) acetate◆
ΔrG 63.1 kJ/mol K 0.88 × 10−11 pK 11.05 - Pb(CH3COO)2Un-ionized aqueous solution + 2H2OLiquidPb(OH)2Crystalline solid + 2CH3COOHIonized 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 | – | 63.1 | – | – |
per 1 mol of | – | 63.1 | – | – |
per 1 mol of | – | 31.6 | – | – |
per 1 mol of | – | 63.1 | – | – |
per 1 mol of | – | 31.6 | – | – |
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(CH3COO)2 (cr) | -963.83[1] | – | – | – |
| Pb(CH3COO)2 (ai) | -973.6[1] | -763.04[1] | 182.8[1] | – |
| Pb(CH3COO)2 (ao) | – | -779.7[1] | – | – |
| Pb(CH3COO)2 (cr) 3 hydrate | -1851.50[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] |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution, (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] | – | – | – |
| CH3COOH (l) | -484.5[1] | -389.9[1] | 159.8[1] | 124.3[1] |
| CH3COOH (g) | -432.25[1] | -374.0[1] | 282.5[1] | 66.5[1] |
| CH3COOH (ai) | -486.01[1] | -369.31[1] | 86.6[1] | -6.3[1] |
| CH3COOH (ao) | -485.76[1] | -396.46[1] | 178.7[1] | – |
* (cr):Crystalline solid, (l):Liquid, (g):Gas, (ai):Ionized aqueous solution, (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°, -963.83 kJ · mol−1
- ^ ΔfH°, -973.6 kJ · mol−1
- ^ ΔfG°, -763.04 kJ · mol−1
- ^ S°, 182.8 J · K−1 · mol−1
- ^ ΔfG°, -779.7 kJ · mol−1
- ^ ΔfH°, -1851.50 kJ · 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°, -484.5 kJ · mol−1
- ^ ΔfG°, -389.9 kJ · mol−1
- ^ S°, 159.8 J · K−1 · mol−1
- ^ Cp°, 124.3 J · K−1 · mol−1
- ^ ΔfH°, -432.25 kJ · mol−1
- ^ ΔfG°, -374.0 kJ · mol−1
- ^ S°, 282.5 J · K−1 · mol−1
- ^ Cp°, 66.5 J · K−1 · mol−1
- ^ ΔfH°, -486.01 kJ · mol−1
- ^ ΔfG°, -369.31 kJ · mol−1
- ^ S°, 86.6 J · K−1 · mol−1
- ^ Cp°, -6.3 J · K−1 · mol−1
- ^ ΔfH°, -485.76 kJ · mol−1
- ^ ΔfG°, -396.46 kJ · mol−1
- ^ S°, 178.7 J · K−1 · mol−1