PbF2 + 2LiOH → 2LiF + Pb(OH)2
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The reaction of lead(II) fluoride and lithium hydroxide yields lithium fluoride and lead(II) hydroxide. 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 lithium hydroxide
General equation
- Reaction of salt of weak base and strong base
- Salt of weak baseBrønsted acid + Strong baseBrønsted base ⟶ Salt of strong baseConjugate acid + Weak baseConjugate base + (H2O)
Oxidation state of each atom
- Reaction of lead(II) fluoride and lithium hydroxide
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| PbF2 | Lead(II) fluoride | 1 | Brønsted acid | Salt of weak base |
| LiOH | Lithium hydroxide | 2 | Brønsted base | Strong base |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| LiF | Lithium fluoride | 2 | Conjugate acid | Salt of strong base |
| Pb(OH)2 | Lead(II) hydroxide | 1 | Conjugate base | Weak base |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of lead(II) fluoride and lithium hydroxide◆
ΔrG −132.6 kJ/mol K 1.70 × 1023 pK −23.23
| 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 | – | −132.6 | – | – |
per 1 mol of | – | −132.6 | – | – |
per 1 mol of | – | −66.30 | – | – |
per 1 mol of | – | −66.30 | – | – |
per 1 mol of | – | −132.6 | – | – |
Changes in standard condition (2)
- Reaction of lead(II) fluoride and lithium 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 | −114.0 | – | – | – |
per 1 mol of | −114.0 | – | – | – |
per 1 mol of | −57.00 | – | – | – |
per 1 mol of | −57.00 | – | – | – |
per 1 mol of | −114.0 | – | – | – |
Changes in aqueous solution (1)
- Reaction of lead(II) fluoride and lithium hydroxide◆
ΔrG −129.9 kJ/mol K 5.72 × 1022 pK −22.76
| 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 | – | −129.9 | – | – |
per 1 mol of | – | −129.9 | – | – |
per 1 mol of | – | −64.95 | – | – |
per 1 mol of | – | −64.95 | – | – |
per 1 mol of | – | −129.9 | – | – |
Changes in aqueous solution (2)
- Reaction of lead(II) fluoride and lithium hydroxide◆
ΔrG −127.4 kJ/mol K 2.09 × 1022 pK −22.32
| 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 | – | −127.4 | – | – |
per 1 mol of | – | −127.4 | – | – |
per 1 mol of | – | −63.70 | – | – |
per 1 mol of | – | −63.70 | – | – |
per 1 mol of | – | −127.4 | – | – |
Changes in aqueous solution (3)
- Reaction of lead(II) fluoride and lithium hydroxide◆
ΔrG −109.4 kJ/mol K 1.47 × 1019 pK −19.17
| 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 | – | −109.4 | – | – |
per 1 mol of | – | −109.4 | – | – |
per 1 mol of | – | −54.70 | – | – |
per 1 mol of | – | −54.70 | – | – |
per 1 mol of | – | −109.4 | – | – |
Changes in aqueous solution (4)
- Reaction of lead(II) fluoride and lithium hydroxide◆
ΔrG −106.9 kJ/mol K 5.35 × 1018 pK −18.73
| 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 | – | −106.9 | – | – |
per 1 mol of | – | −106.9 | – | – |
per 1 mol of | – | −53.45 | – | – |
per 1 mol of | – | −53.45 | – | – |
per 1 mol of | – | −106.9 | – | – |
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] | – | – |
| LiOH (cr) | -484.93[1] | -438.95[1] | 42.80[1] | 49.66[1] |
| LiOH (g) | -238.1[1] | -242.3[1] | 210.90[1] | 46.02[1] |
| LiOH (ai) | -508.48[1] | -450.58[1] | 2.80[1] | -79.9[1] |
| LiOH (ao) | -508.4[1] | -451.8[1] | 7.1[1] | – |
| LiOH (cr) 1 hydrate | -788.01[1] | -680.95[1] | 71.21[1] | 79.50[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 |
|---|---|---|---|---|
| LiF (cr) | -615.97[1] | -587.71[1] | 35.65[1] | 41.59[1] |
| LiF (g) | -339.82[1] | -360.64[1] | 200.297[1] | 31.30[1] |
| LiF (ai) | -611.12[1] | -571.9[1] | -0.4[1] | -38.07[1] |
| Pb(OH)2 (cr) | – | -452.2[1] | – | – |
| Pb(OH)2 (cr) precipitated | -515.9[1] | – | – | – |
* (cr):Crystalline solid, (g):Gas, (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)
- ^ 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°, -484.93 kJ · mol−1
- ^ ΔfG°, -438.95 kJ · mol−1
- ^ S°, 42.80 J · K−1 · mol−1
- ^ Cp°, 49.66 J · K−1 · mol−1
- ^ ΔfH°, -238.1 kJ · mol−1
- ^ ΔfG°, -242.3 kJ · mol−1
- ^ S°, 210.90 J · K−1 · mol−1
- ^ Cp°, 46.02 J · K−1 · mol−1
- ^ ΔfH°, -508.48 kJ · mol−1
- ^ ΔfG°, -450.58 kJ · mol−1
- ^ S°, 2.80 J · K−1 · mol−1
- ^ Cp°, -79.9 J · K−1 · mol−1
- ^ ΔfH°, -508.4 kJ · mol−1
- ^ ΔfG°, -451.8 kJ · mol−1
- ^ S°, 7.1 J · K−1 · mol−1
- ^ ΔfH°, -788.01 kJ · mol−1
- ^ ΔfG°, -680.95 kJ · mol−1
- ^ S°, 71.21 J · K−1 · mol−1
- ^ Cp°, 79.50 J · K−1 · mol−1
- ^ ΔfH°, -615.97 kJ · mol−1
- ^ ΔfG°, -587.71 kJ · mol−1
- ^ S°, 35.65 J · K−1 · mol−1
- ^ Cp°, 41.59 J · K−1 · mol−1
- ^ ΔfH°, -339.82 kJ · mol−1
- ^ ΔfG°, -360.64 kJ · mol−1
- ^ S°, 200.297 J · K−1 · mol−1
- ^ Cp°, 31.30 J · K−1 · mol−1
- ^ ΔfH°, -611.12 kJ · mol−1
- ^ ΔfG°, -571.9 kJ · mol−1
- ^ S°, -0.4 J · K−1 · mol−1
- ^ Cp°, -38.07 J · K−1 · mol−1
- ^ ΔfG°, -452.2 kJ · mol−1
- ^ ΔfH°, -515.9 kJ · mol−1