PbF2 + 2H2O → Pb(OH)2 + 2HF↑
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- Hydrolysis of lead(II) fluoride
The reaction of lead(II) fluoride and water yields lead(II) hydroxide and hydrogen fluoride. This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Hydrolysis of lead(II) fluoride
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) fluoride
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| PbF2 | Lead(II) fluoride | 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 |
| HF | Hydrogen fluoride | 2 | Conjugate acid | Acid |
Thermodynamic changes
Changes in standard condition (1)
- Hydrolysis of lead(II) fluoride◆
ΔrG 92.8 kJ/mol K 0.55 × 10−16 pK 16.26
| 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 | – | 92.8 | – | – |
per 1 mol of | – | 92.8 | – | – |
per 1 mol of | – | 46.4 | – | – |
per 1 mol of | – | 92.8 | – | – |
per 1 mol of | – | 46.4 | – | – |
Changes in standard condition (2)
- Hydrolysis of lead(II) fluoride
| 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 | 177.6 | – | – | – |
per 1 mol of | 177.6 | – | – | – |
per 1 mol of | 88.80 | – | – | – |
per 1 mol of | 177.6 | – | – | – |
per 1 mol of | 88.80 | – | – | – |
Changes in aqueous solution (1)
- Hydrolysis of lead(II) fluoride◆
ΔrG 72.3 kJ/mol K 0.22 × 10−12 pK 12.67
| 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 | – | 72.3 | – | – |
per 1 mol of | – | 72.3 | – | – |
per 1 mol of | – | 36.1 | – | – |
per 1 mol of | – | 72.3 | – | – |
per 1 mol of | – | 36.1 | – | – |
Changes in aqueous solution (2)
- Hydrolysis of lead(II) fluoride◆
ΔrG 25.0 kJ/mol K 0.42 × 10−4 pK 4.38
| 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 | – | 25.0 | – | – |
per 1 mol of | – | 25.0 | – | – |
per 1 mol of | – | 12.5 | – | – |
per 1 mol of | – | 25.0 | – | – |
per 1 mol of | – | 12.5 | – | – |
Changes in aqueous solution (3)
- Hydrolysis of lead(II) fluoride◆
ΔrG 25.0 kJ/mol K 0.42 × 10−4 pK 4.38
| 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 | – | 25.0 | – | – |
per 1 mol of | – | 25.0 | – | – |
per 1 mol of | – | 12.5 | – | – |
per 1 mol of | – | 25.0 | – | – |
per 1 mol of | – | 12.5 | – | – |
Changes in aqueous solution (4)
- Hydrolysis of lead(II) fluoride◆
ΔrG 92.8 kJ/mol K 0.55 × 10−16 pK 16.26
| 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 | – | 92.8 | – | – |
per 1 mol of | – | 92.8 | – | – |
per 1 mol of | – | 46.4 | – | – |
per 1 mol of | – | 92.8 | – | – |
per 1 mol of | – | 46.4 | – | – |
Changes in aqueous solution (5)
- Hydrolysis of lead(II) fluoride◆
ΔrG 45.5 kJ/mol K 0.11 × 10−7 pK 7.97
| 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 | – | 45.5 | – | – |
per 1 mol of | – | 45.5 | – | – |
per 1 mol of | – | 22.8 | – | – |
per 1 mol of | – | 45.5 | – | – |
per 1 mol of | – | 22.8 | – | – |
Changes in aqueous solution (6)
- Hydrolysis of lead(II) fluoride◆
ΔrG 45.5 kJ/mol K 0.11 × 10−7 pK 7.97
| 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 | – | 45.5 | – | – |
per 1 mol of | – | 45.5 | – | – |
per 1 mol of | – | 22.8 | – | – |
per 1 mol of | – | 45.5 | – | – |
per 1 mol of | – | 22.8 | – | – |
Changes in aqueous solution (7)
- Hydrolysis of lead(II) fluoride◆
ΔrG 61.1 kJ/mol K 0.20 × 10−10 pK 10.70
| 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 | – | 61.1 | – | – |
per 1 mol of | – | 61.1 | – | – |
per 1 mol of | – | 30.6 | – | – |
per 1 mol of | – | 61.1 | – | – |
per 1 mol of | – | 30.6 | – | – |
Changes in aqueous solution (8)
- Hydrolysis of lead(II) fluoride◆
ΔrG 81.6 kJ/mol K 0.51 × 10−14 pK 14.30
| 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 | – | 81.6 | – | – |
per 1 mol of | – | 81.6 | – | – |
per 1 mol of | – | 40.8 | – | – |
per 1 mol of | – | 81.6 | – | – |
per 1 mol of | – | 40.8 | – | – |
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 |
|---|---|---|---|---|
| PbF2 (cr) | -664.0[1] | -617.1[1] | 110.5[1] | – |
| PbF2 (ai) | -666.9[1] | -582.00[1] | -17.2[1] | – |
| PbF2 (ao) | – | -596.6[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] | – | – | – |
| HF (l) x denotes undetermined zero point entropy | -299.78[1] | – | 75.40+x[1] | – |
| HF (g) | -271.1[1] | -273.2[1] | 173.779[1] | 29.133[1] |
| HF (ai) | -332.63[1] | -278.79[1] | -13.8[1] | -106.7[1] |
| HF (ao) | -320.08[1] | -296.82[1] | 88.7[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°, -664.0 kJ · mol−1
- ^ ΔfG°, -617.1 kJ · mol−1
- ^ S°, 110.5 J · K−1 · mol−1
- ^ ΔfH°, -666.9 kJ · mol−1
- ^ ΔfG°, -582.00 kJ · mol−1
- ^ S°, -17.2 J · K−1 · mol−1
- ^ ΔfG°, -596.6 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°, -299.78 kJ · mol−1
- ^ S°, 75.40+x J · K−1 · mol−1
- ^ ΔfH°, -271.1 kJ · mol−1
- ^ ΔfG°, -273.2 kJ · mol−1
- ^ S°, 173.779 J · K−1 · mol−1
- ^ Cp°, 29.133 J · K−1 · mol−1
- ^ ΔfH°, -332.63 kJ · mol−1
- ^ ΔfG°, -278.79 kJ · mol−1
- ^ S°, -13.8 J · K−1 · mol−1
- ^ Cp°, -106.7 J · K−1 · mol−1
- ^ ΔfH°, -320.08 kJ · mol−1
- ^ ΔfG°, -296.82 kJ · mol−1
- ^ S°, 88.7 J · K−1 · mol−1