HBr + AgOH → AgBr + H2O
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- Reaction of hydrogen bromide and silver(I) hydroxide
The reaction of hydrogen bromide and silver(I) hydroxide yields silver(I) bromide and water. This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of hydrogen bromide and silver(I) 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 strong base
- Strong acidBrønsted acid + Strong baseBrønsted base ⟶ Salt of strong acid and strong baseConjugate base + (H2O)(Conjugate acid)
Oxidation state of each atom
- Reaction of hydrogen bromide and silver(I) hydroxide
Reactants
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
HBr | Hydrogen bromide | 1 | Brønsted acid | Acid Strong acid |
AgOH | Silver(I) hydroxide | 1 | Brønsted base | Base Hydroxide base Strong base |
Products
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
AgBr | Silver(I) bromide | 1 | Conjugate base | Salt Salt of strong acid and strong base |
H2O | Water | 1 | Conjugate acid | Water |
Thermodynamic changes
Changes in aqueous solution (1)
- Reaction of hydrogen bromide and silver(I) hydroxide◆
ΔrG −79.89 kJ/mol K 9.91 × 1013 pK −14.00
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 | −55.85 | −79.89 | 80.8 | 223.8 |
per 1 mol of | −55.85 | −79.89 | 80.8 | 223.8 |
per 1 mol of Silver(I) hydroxide | −55.85 | −79.89 | 80.8 | 223.8 |
per 1 mol of | −55.85 | −79.89 | 80.8 | 223.8 |
per 1 mol of | −55.85 | −79.89 | 80.8 | 223.8 |
Changes in aqueous solution (2)
- Reaction of hydrogen bromide and silver(I) hydroxide◆
ΔrG −104.0 kJ/mol K 1.66 × 1018 pK −18.22
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 | – | −104.0 | – | – |
per 1 mol of | – | −104.0 | – | – |
per 1 mol of Silver(I) hydroxide | – | −104.0 | – | – |
per 1 mol of | – | −104.0 | – | – |
per 1 mol of | – | −104.0 | – | – |
Changes in aqueous solution (3)
- Reaction of hydrogen bromide and silver(I) hydroxide◆
ΔrG −68.0 kJ/mol K 8.19 × 1011 pK −11.91
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 | – | −68.0 | – | – |
per 1 mol of | – | −68.0 | – | – |
per 1 mol of Silver(I) hydroxide | – | −68.0 | – | – |
per 1 mol of | – | −68.0 | – | – |
per 1 mol of | – | −68.0 | – | – |
Changes in aqueous solution (4)
- Reaction of hydrogen bromide and silver(I) hydroxide◆
ΔrG −92.2 kJ/mol K 1.42 × 1016 pK −16.15
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 | – | −92.2 | – | – |
per 1 mol of | – | −92.2 | – | – |
per 1 mol of Silver(I) hydroxide | – | −92.2 | – | – |
per 1 mol of | – | −92.2 | – | – |
per 1 mol of | – | −92.2 | – | – |
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 |
---|---|---|---|---|
HBr (g) | -36.40[1] | -53.45[1] | 198.695[1] | 29.142[1] |
HBr (ai) | -121.55[1] | -103.96[1] | 82.4[1] | -141.8[1] |
AgOH (ai) | -124.415[1] | -80.137[1] | 61.92[1] | -126.8[1] |
AgOH (ao) | – | -92.0[1] | – | – |
* (g):Gas, (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution
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 |
---|---|---|---|---|
AgBr (cr) | -100.37[1] | -96.90[1] | 107.1[1] | 52.38[1] |
AgBr (ai) | -15.98[1] | -26.86[1] | 155.2[1] | -120.1[1] |
AgBr (ao) | – | -51.0[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°, -36.40 kJ · mol−1
- ^ ΔfG°, -53.45 kJ · mol−1
- ^ S°, 198.695 J · K−1 · mol−1
- ^ Cp°, 29.142 J · K−1 · mol−1
- ^ ΔfH°, -121.55 kJ · mol−1
- ^ ΔfG°, -103.96 kJ · mol−1
- ^ S°, 82.4 J · K−1 · mol−1
- ^ Cp°, -141.8 J · K−1 · mol−1
- ^ ΔfH°, -124.415 kJ · mol−1
- ^ ΔfG°, -80.137 kJ · mol−1
- ^ S°, 61.92 J · K−1 · mol−1
- ^ Cp°, -126.8 J · K−1 · mol−1
- ^ ΔfG°, -92.0 kJ · mol−1
- ^ ΔfH°, -100.37 kJ · mol−1
- ^ ΔfG°, -96.90 kJ · mol−1
- ^ S°, 107.1 J · K−1 · mol−1
- ^ Cp°, 52.38 J · K−1 · mol−1
- ^ ΔfH°, -15.98 kJ · mol−1
- ^ ΔfG°, -26.86 kJ · mol−1
- ^ S°, 155.2 J · K−1 · mol−1
- ^ Cp°, -120.1 J · K−1 · mol−1
- ^ ΔfG°, -51.0 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