2HI + Pb(OH)2 → PbI2 + 2H2O
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- Reaction of hydrogen iodide and lead(II) hydroxide
The reaction of hydrogen iodide and lead(II) hydroxide yields lead(II) iodide 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 strong acid and weak base
- Reaction of acid and amphoteric hydroxide
- Reaction of strong acid and amphoteric hydroxide
Table of contents
Reaction data
Chemical equation
- Reaction of hydrogen iodide 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 strong acid and weak base
- Strong acidBrønsted acid + Weak baseBrønsted base ⟶ Salt of strong 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 strong acid and amphoteric hydroxide
- Strong acidBrønsted acid + Amphoteric hydroxideBrønsted base ⟶ Salt of strong acid and weak baseConjugate base + H2OConjugate acid
Oxidation state of each atom
- Reaction of hydrogen iodide and lead(II) hydroxide
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| HI | Hydrogen iodide | 2 | Brønsted acid | Acid Strong 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 |
|---|---|---|---|---|
| PbI2 | Lead(II) iodide | 1 | Conjugate base | Salt Salt of strong acid and weak base Salt of weak base |
| H2O | Water | 2 | Conjugate acid | Water |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of hydrogen iodide and lead(II) hydroxide◆
ΔrG −199.1 kJ/mol K 7.60 × 1034 pK −34.88
| 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 | – | −199.1 | – | – |
per 1 mol of | – | −99.55 | – | – |
per 1 mol of | – | −199.1 | – | – |
per 1 mol of | – | −199.1 | – | – |
per 1 mol of | – | −99.55 | – | – |
Changes in standard condition (2)
- Reaction of hydrogen iodide 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 | −284.2 | – | – | – |
per 1 mol of | −142.1 | – | – | – |
per 1 mol of | −284.2 | – | – | – |
per 1 mol of | −284.2 | – | – | – |
per 1 mol of | −142.1 | – | – | – |
Changes in aqueous solution (1)
- Reaction of hydrogen iodide and lead(II) hydroxide◆
ΔrG −46.5 kJ/mol K 1.40 × 108 pK −8.15
| 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 | – | −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 hydrogen iodide and lead(II) hydroxide◆
ΔrG −62.4 kJ/mol K 8.55 × 1010 pK −10.93
| 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 | – | −62.4 | – | – |
per 1 mol of | – | −31.2 | – | – |
per 1 mol of | – | −62.4 | – | – |
per 1 mol of | – | −62.4 | – | – |
per 1 mol of | – | −31.2 | – | – |
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 |
|---|---|---|---|---|
| HI (g) | 26.48[1] | 1.70[1] | 206.594[1] | 29.158[1] |
| HI (ai) | -55.19[1] | -51.57[1] | 111.3[1] | -142.3[1] |
| Pb(OH)2 (cr) | – | -452.2[1] | – | – |
| Pb(OH)2 (cr) precipitated | -515.9[1] | – | – | – |
* (g):Gas, (ai):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 |
|---|---|---|---|---|
| PbI2 (cr) | -175.48[1] | -173.64[1] | 174.85[1] | 77.36[1] |
| PbI2 (ai) | -112.1[1] | -127.57[1] | 233.0[1] | – |
| PbI2 (ao) | – | -143.5[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°, 26.48 kJ · mol−1
- ^ ΔfG°, 1.70 kJ · mol−1
- ^ S°, 206.594 J · K−1 · mol−1
- ^ Cp°, 29.158 J · K−1 · mol−1
- ^ ΔfH°, -55.19 kJ · mol−1
- ^ ΔfG°, -51.57 kJ · mol−1
- ^ S°, 111.3 J · K−1 · mol−1
- ^ Cp°, -142.3 J · K−1 · mol−1
- ^ ΔfG°, -452.2 kJ · mol−1
- ^ ΔfH°, -515.9 kJ · mol−1
- ^ ΔfH°, -175.48 kJ · mol−1
- ^ ΔfG°, -173.64 kJ · mol−1
- ^ S°, 174.85 J · K−1 · mol−1
- ^ Cp°, 77.36 J · K−1 · mol−1
- ^ ΔfH°, -112.1 kJ · mol−1
- ^ ΔfG°, -127.57 kJ · mol−1
- ^ S°, 233.0 J · K−1 · mol−1
- ^ ΔfG°, -143.5 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