PbF2 + 2HCl → PbCl2 + 2HF
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The reaction of lead(II) fluoride and hydrogen chloride yields lead(II) chloride and hydrogen fluoride. This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of lead(II) fluoride and hydrogen chloride
General equation
- Salt of weak acidBrønsted base + Strong acidBrønsted acid ⟶ Salt of strong acidConjugate base + Weak acidConjugate acid
Oxidation state of each atom
- Reaction of lead(II) fluoride and hydrogen chloride
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| PbF2 | Lead(II) fluoride | 1 | Brønsted base | Salt of weak acid |
| HCl | Hydrogen chloride | 2 | Brønsted acid | Strong acid |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| PbCl2 | Lead(II) chloride | 1 | Conjugate base | Salt of strong acid |
| HF | Hydrogen fluoride | 2 | Conjugate acid | Weak acid |
Thermodynamic changes
Changes in standard condition
- Reaction of lead(II) fluoride and hydrogen chloride◆
ΔrG −52.8 kJ/mol K 1.78 × 109 pK −9.25
| 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 | −53.0 | −52.8 | −0.8 | – |
per 1 mol of | −53.0 | −52.8 | −0.80 | – |
per 1 mol of | −26.5 | −26.4 | −0.40 | – |
per 1 mol of | −53.0 | −52.8 | −0.80 | – |
per 1 mol of | −26.5 | −26.4 | −0.40 | – |
Changes in aqueous solution (1)
- Reaction of lead(II) fluoride and hydrogen chloride◆
ΔrG 25.8 kJ/mol K 0.30 × 10−4 pK 4.52
| 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 | – | 25.8 | – | – |
per 1 mol of | – | 25.8 | – | – |
per 1 mol of | – | 12.9 | – | – |
per 1 mol of | – | 25.8 | – | – |
per 1 mol of | – | 12.9 | – | – |
Changes in aqueous solution (2)
- Reaction of lead(II) fluoride and hydrogen chloride◆
ΔrG −21.4 kJ/mol K 5.61 × 103 pK −3.75
| 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 | – | −21.4 | – | – |
per 1 mol of | – | −21.4 | – | – |
per 1 mol of | – | −10.7 | – | – |
per 1 mol of | – | −21.4 | – | – |
per 1 mol of | – | −10.7 | – | – |
Changes in aqueous solution (3)
- Reaction of lead(II) fluoride and hydrogen chloride◆
ΔrG −21.4 kJ/mol K 5.61 × 103 pK −3.75
| 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 | – | −21.4 | – | – |
per 1 mol of | – | −21.4 | – | – |
per 1 mol of | – | −10.7 | – | – |
per 1 mol of | – | −21.4 | – | – |
per 1 mol of | – | −10.7 | – | – |
Changes in aqueous solution (4)
- Reaction of lead(II) fluoride and hydrogen chloride◆
ΔrG 15.5 kJ/mol K 0.19 × 10−2 pK 2.72
| 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 | – | 15.5 | – | – |
per 1 mol of | – | 15.5 | – | – |
per 1 mol of | – | 7.75 | – | – |
per 1 mol of | – | 15.5 | – | – |
per 1 mol of | – | 7.75 | – | – |
Changes in aqueous solution (5)
- Reaction of lead(II) fluoride and hydrogen chloride◆
ΔrG −31.7 kJ/mol K 3.58 × 105 pK −5.55
| 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 | – | −31.7 | – | – |
per 1 mol of | – | −31.7 | – | – |
per 1 mol of | – | −15.8 | – | – |
per 1 mol of | – | −31.7 | – | – |
per 1 mol of | – | −15.8 | – | – |
Changes in aqueous solution (6)
- Reaction of lead(II) fluoride and hydrogen chloride◆
ΔrG −31.7 kJ/mol K 3.58 × 105 pK −5.55
| 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 | – | −31.7 | – | – |
per 1 mol of | – | −31.7 | – | – |
per 1 mol of | – | −15.8 | – | – |
per 1 mol of | – | −31.7 | – | – |
per 1 mol of | – | −15.8 | – | – |
Changes in aqueous solution (7)
- Reaction of lead(II) fluoride and hydrogen chloride◆
ΔrG 46.3 kJ/mol K 0.77 × 10−8 pK 8.11
| 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 | 120.1 | 46.3 | 247.5 | – |
per 1 mol of | 120.1 | 46.3 | 247.5 | – |
per 1 mol of | 60.05 | 23.1 | 123.8 | – |
per 1 mol of | 120.1 | 46.3 | 247.5 | – |
per 1 mol of | 60.05 | 23.1 | 123.8 | – |
Changes in aqueous solution (8)
- Reaction of lead(II) fluoride and hydrogen chloride◆
ΔrG −0.9 kJ/mol K 1.44 × 100 pK −0.16
| 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 | 22.2 | −0.9 | 77.3 | – |
per 1 mol of | 22.2 | −0.90 | 77.3 | – |
per 1 mol of | 11.1 | −0.45 | 38.6 | – |
per 1 mol of | 22.2 | −0.90 | 77.3 | – |
per 1 mol of | 11.1 | −0.45 | 38.6 | – |
Changes in aqueous solution (9)
- Reaction of lead(II) fluoride and hydrogen chloride◆
ΔrG −0.9 kJ/mol K 1.44 × 100 pK −0.16
| 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 | 22.2 | −0.9 | 77.3 | – |
per 1 mol of | 22.2 | −0.90 | 77.3 | – |
per 1 mol of | 11.1 | −0.45 | 38.6 | – |
per 1 mol of | 22.2 | −0.90 | 77.3 | – |
per 1 mol of | 11.1 | −0.45 | 38.6 | – |
Changes in aqueous solution (10)
- Reaction of lead(II) fluoride and hydrogen chloride◆
ΔrG 36.0 kJ/mol K 0.49 × 10−6 pK 6.31
| 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 | – | 36.0 | – | – |
per 1 mol of | – | 36.0 | – | – |
per 1 mol of | – | 18.0 | – | – |
per 1 mol of | – | 36.0 | – | – |
per 1 mol of | – | 18.0 | – | – |
Changes in aqueous solution (11)
- Reaction of lead(II) fluoride and hydrogen chloride◆
ΔrG −11.2 kJ/mol K 9.17 × 101 pK −1.96
| 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 | – | −11.2 | – | – |
per 1 mol of | – | −11.2 | – | – |
per 1 mol of | – | −5.60 | – | – |
per 1 mol of | – | −11.2 | – | – |
per 1 mol of | – | −5.60 | – | – |
Changes in aqueous solution (12)
- Reaction of lead(II) fluoride and hydrogen chloride◆
ΔrG −11.2 kJ/mol K 9.17 × 101 pK −1.96
| 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 | – | −11.2 | – | – |
per 1 mol of | – | −11.2 | – | – |
per 1 mol of | – | −5.60 | – | – |
per 1 mol of | – | −11.2 | – | – |
per 1 mol of | – | −5.60 | – | – |
Changes in aqueous solution (13)
- Reaction of lead(II) fluoride and hydrogen chloride◆
ΔrG 14.6 kJ/mol K 0.28 × 10−2 pK 2.56
| 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 | – | 14.6 | – | – |
per 1 mol of | – | 14.6 | – | – |
per 1 mol of | – | 7.30 | – | – |
per 1 mol of | – | 14.6 | – | – |
per 1 mol of | – | 7.30 | – | – |
Changes in aqueous solution (14)
- Reaction of lead(II) fluoride and hydrogen chloride◆
ΔrG 4.3 kJ/mol K 0.18 × 100 pK 0.75
| 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 | – | 4.3 | – | – |
per 1 mol of | – | 4.3 | – | – |
per 1 mol of | – | 2.1 | – | – |
per 1 mol of | – | 4.3 | – | – |
per 1 mol of | – | 2.1 | – | – |
Changes in aqueous solution (15)
- Reaction of lead(II) fluoride and hydrogen chloride◆
ΔrG 35.1 kJ/mol K 0.71 × 10−6 pK 6.15
| 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 | −2.9 | 35.1 | −127.7 | – |
per 1 mol of | −2.9 | 35.1 | −127.7 | – |
per 1 mol of | −1.4 | 17.6 | −63.85 | – |
per 1 mol of | −2.9 | 35.1 | −127.7 | – |
per 1 mol of | −1.4 | 17.6 | −63.85 | – |
Changes in aqueous solution (16)
- Reaction of lead(II) fluoride and hydrogen chloride◆
ΔrG 24.8 kJ/mol K 0.45 × 10−4 pK 4.34
| 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 | – | 24.8 | – | – |
per 1 mol of | – | 24.8 | – | – |
per 1 mol of | – | 12.4 | – | – |
per 1 mol of | – | 24.8 | – | – |
per 1 mol of | – | 12.4 | – | – |
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 |
|---|---|---|---|---|
| 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] | – | – |
| HCl (g) | -92.307[1] | -95.299[1] | 186.908[1] | 29.12[1] |
| HCl (ai) | -167.159[1] | -131.228[1] | 56.5[1] | -136.4[1] |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution, (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 |
|---|---|---|---|---|
| PbCl2 (cr) | -359.41[1] | -314.10[1] | 136.0[1] | – |
| PbCl2 (ai) | -336.0[1] | -286.86[1] | 123.4[1] | – |
| PbCl2 (ao) | – | -297.16[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, (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°, -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°, -92.307 kJ · mol−1
- ^ ΔfG°, -95.299 kJ · mol−1
- ^ S°, 186.908 J · K−1 · mol−1
- ^ Cp°, 29.12 J · K−1 · mol−1
- ^ ΔfH°, -167.159 kJ · mol−1
- ^ ΔfG°, -131.228 kJ · mol−1
- ^ S°, 56.5 J · K−1 · mol−1
- ^ Cp°, -136.4 J · K−1 · mol−1
- ^ ΔfH°, -359.41 kJ · mol−1
- ^ ΔfG°, -314.10 kJ · mol−1
- ^ S°, 136.0 J · K−1 · mol−1
- ^ ΔfH°, -336.0 kJ · mol−1
- ^ ΔfG°, -286.86 kJ · mol−1
- ^ S°, 123.4 J · K−1 · mol−1
- ^ ΔfG°, -297.16 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