NH4F + HBr → NH4Br + HF
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The reaction of ammonium fluoride and hydrogen bromide yields ammonium bromide and hydrogen fluoride. This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of ammonium fluoride and hydrogen bromide
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 ammonium fluoride and hydrogen bromide
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| NH4F | Ammonium fluoride | 1 | Brønsted base | Salt of weak acid |
| HBr | Hydrogen bromide | 1 | Brønsted acid | Strong acid |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| NH4Br | Ammonium bromide | 1 | Conjugate base | Salt of strong acid |
| HF | Hydrogen fluoride | 1 | Conjugate acid | Weak acid |
Thermodynamic changes
Changes in standard condition
- Reaction of ammonium fluoride and hydrogen bromide◆
ΔrG −46.3 kJ/mol K 1.29 × 108 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 | −41.6 | −46.3 | 16 | 31 |
per 1 mol of | −41.6 | −46.3 | 16 | 31 |
per 1 mol of | −41.6 | −46.3 | 16 | 31 |
per 1 mol of | −41.6 | −46.3 | 16 | 31 |
per 1 mol of | −41.6 | −46.3 | 16 | 31 |
Changes in aqueous solution (1)
- Reaction of ammonium fluoride and hydrogen bromide◆
ΔrG 5.6 kJ/mol K 0.10 × 100 pK 0.98
| 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 | 61.5 | 5.6 | 187.6 | 135.8 |
per 1 mol of | 61.5 | 5.6 | 187.6 | 135.8 |
per 1 mol of | 61.5 | 5.6 | 187.6 | 135.8 |
per 1 mol of | 61.5 | 5.6 | 187.6 | 135.8 |
per 1 mol of | 61.5 | 5.6 | 187.6 | 135.8 |
Changes in aqueous solution (2)
- Reaction of ammonium fluoride and hydrogen bromide◆
ΔrG −18.03 kJ/mol K 1.44 × 103 pK −3.16
| 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 | 12.56 | −18.03 | 102.5 | – |
per 1 mol of | 12.56 | −18.03 | 102.5 | – |
per 1 mol of | 12.56 | −18.03 | 102.5 | – |
per 1 mol of | 12.56 | −18.03 | 102.5 | – |
per 1 mol of | 12.56 | −18.03 | 102.5 | – |
Changes in aqueous solution (3)
- Reaction of ammonium fluoride and hydrogen bromide◆
ΔrG −18.03 kJ/mol K 1.44 × 103 pK −3.16
| 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 | 12.56 | −18.03 | 102.5 | – |
per 1 mol of | 12.56 | −18.03 | 102.5 | – |
per 1 mol of | 12.56 | −18.03 | 102.5 | – |
per 1 mol of | 12.56 | −18.03 | 102.5 | – |
per 1 mol of | 12.56 | −18.03 | 102.5 | – |
Changes in aqueous solution (4)
- Reaction of ammonium fluoride and hydrogen bromide◆
ΔrG 0.00 kJ/mol K 1.00 × 100 pK 0.00
| 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 | 0.01 | 0.00 | 0.0 | 0.0 |
per 1 mol of | 0.0100 | 0.00 | 0.0 | 0.0 |
per 1 mol of | 0.0100 | 0.00 | 0.0 | 0.0 |
per 1 mol of | 0.0100 | 0.00 | 0.0 | 0.0 |
per 1 mol of | 0.0100 | 0.00 | 0.0 | 0.0 |
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 |
|---|---|---|---|---|
| NH4F (cr) | -463.96[1] | -348.68[1] | 71.96[1] | 65.27[1] |
| NH4F (ai) | -465.14[1] | -358.09[1] | 99.6[1] | -26.8[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] |
* (cr):Crystalline solid, (ai):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 |
|---|---|---|---|---|
| NH4Br (cr) | -270.83[1] | -175.2[1] | 113[1] | 96[1] |
| NH4Br (ai) | -254.05[1] | -183.26[1] | 195.8[1] | -61.9[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, (ai):Ionized aqueous solution, (l):Liquid, (g):Gas, (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°, -463.96 kJ · mol−1
- ^ ΔfG°, -348.68 kJ · mol−1
- ^ S°, 71.96 J · K−1 · mol−1
- ^ Cp°, 65.27 J · K−1 · mol−1
- ^ ΔfH°, -465.14 kJ · mol−1
- ^ ΔfG°, -358.09 kJ · mol−1
- ^ S°, 99.6 J · K−1 · mol−1
- ^ Cp°, -26.8 J · K−1 · mol−1
- ^ 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°, -270.83 kJ · mol−1
- ^ ΔfG°, -175.2 kJ · mol−1
- ^ S°, 113. J · K−1 · mol−1
- ^ Cp°, 96. J · K−1 · mol−1
- ^ ΔfH°, -254.05 kJ · mol−1
- ^ ΔfG°, -183.26 kJ · mol−1
- ^ S°, 195.8 J · K−1 · mol−1
- ^ Cp°, -61.9 J · K−1 · 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