2CH3COOH + Pb(OH)2 → Pb(CH3COO)2 + 2H2O
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The reaction of acetic acid and lead(II) hydroxide yields lead(II) acetate and water. This reaction is an acid-base reaction and is classified as follows:
- Reaction of acid and base
- Reaction of acid and hydroxide base
- Reaction of weak acid and weak base
- Reaction of acid and amphoteric hydroxide
- Reaction of weak acid and amphoteric hydroxide
Table of contents
Reaction data
Chemical equation
- Reaction of acetic acid and lead(II) hydroxide
General equation
- Reaction of acid and base
- AcidBrønsted acid + BaseBrønsted base ⟶ SaltConjugate base + (H2O)(Conjugate acid)
- Reaction of acid and hydroxide base
- AcidBrønsted acid + Hydroxide baseBrønsted base ⟶ SaltConjugate base + H2OConjugate acid
- Reaction of weak acid and weak base
- Weak acidBrønsted acid + Weak baseBrønsted base ⟶ Salt of weak acid and weak baseConjugate base + (H2O)(Conjugate acid)
- Reaction of acid and amphoteric hydroxide
- AcidBrønsted acid + Amphoteric hydroxideBrønsted base ⟶ Salt of weak baseConjugate base + H2OConjugate acid
- Reaction of weak acid and amphoteric hydroxide
- Weak acidBrønsted acid + Amphoteric hydroxideBrønsted base ⟶ Salt of weak acid and weak baseConjugate base + H2OConjugate acid
Oxidation state of each atom
- Reaction of acetic acid and lead(II) hydroxide
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| CH3COOH | Acetic acid | 2 | Brønsted acid | Acid Weak acid |
| Pb(OH)2 | Lead(II) hydroxide | 1 | Brønsted base | Base Hydroxide base Weak base Amphoteric hydroxide |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Pb(CH3COO)2 | Lead(II) acetate | 1 | Conjugate base | Salt Salt of weak acid and weak base Salt of weak base |
| H2O | Water | 2 | Conjugate acid | Water |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of acetic acid and lead(II) hydroxide
| 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)
- Reaction of acetic acid and lead(II) hydroxide
| 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 | −25.3 | – | – | – |
per 1 mol of | −50.6 | – | – | – |
per 1 mol of | −50.6 | – | – | – |
per 1 mol of | −25.3 | – | – | – |
Changes in aqueous solution (1)
- Reaction of acetic acid and lead(II) hydroxide◆
ΔrG −46.5 kJ/mol K 1.40 × 108 pK −8.15 - 2CH3COOHIonized aqueous solution + Pb(OH)2Crystalline solidPb(CH3COO)2Ionized aqueous solution + 2H2OLiquid⟶
| 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 | – | −23.3 | – | – |
per 1 mol of | – | −46.5 | – | – |
per 1 mol of | – | −46.5 | – | – |
per 1 mol of | – | −23.3 | – | – |
Changes in aqueous solution (2)
- Reaction of acetic acid and lead(II) hydroxide◆
ΔrG −63.1 kJ/mol K 1.13 × 1011 pK −11.05 - 2CH3COOHIonized aqueous solution + Pb(OH)2Crystalline solidPb(CH3COO)2Un-ionized aqueous solution + 2H2OLiquid⟶
| 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 | – | −31.6 | – | – |
per 1 mol of | – | −63.1 | – | – |
per 1 mol of | – | −63.1 | – | – |
per 1 mol of | – | −31.6 | – | – |
Changes in aqueous solution (3)
- Reaction of acetic acid and lead(II) hydroxide◆
ΔrG 7.8 kJ/mol K 0.43 × 10−1 pK 1.37 - 2CH3COOHUn-ionized aqueous solution + Pb(OH)2Crystalline solidPb(CH3COO)2Ionized aqueous solution + 2H2OLiquid⟶
| 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 | – | 3.9 | – | – |
per 1 mol of | – | 7.8 | – | – |
per 1 mol of | – | 7.8 | – | – |
per 1 mol of | – | 3.9 | – | – |
Changes in aqueous solution (4)
- Reaction of acetic acid and lead(II) hydroxide◆
ΔrG −8.8 kJ/mol K 3.48 × 101 pK −1.54 - 2CH3COOHUn-ionized aqueous solution + Pb(OH)2Crystalline solidPb(CH3COO)2Un-ionized aqueous solution + 2H2OLiquid⟶
| 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 | – | −4.4 | – | – |
per 1 mol of | – | −8.8 | – | – |
per 1 mol of | – | −8.8 | – | – |
per 1 mol of | – | −4.4 | – | – |
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 |
|---|---|---|---|---|
| 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] | – |
| Pb(OH)2 (cr) | – | -452.2[1] | – | – |
| Pb(OH)2 (cr) precipitated | -515.9[1] | – | – | – |
* (l):Liquid, (g):Gas, (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution, (cr):Crystalline solid
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(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
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°, -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
- ^ ΔfG°, -452.2 kJ · mol−1
- ^ ΔfH°, -515.9 kJ · mol−1
- ^ 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