HF + KOH → KF + H2O
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The reaction of hydrogen fluoride and potassium hydroxide yields potassium fluoride and water. This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of hydrogen fluoride and potassium 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 weak acid and strong base
- Weak acidBrønsted acid + Strong baseBrønsted base ⟶ Salt of weak acid and strong baseConjugate base + (H2O)(Conjugate acid)
Oxidation state of each atom
- Reaction of hydrogen fluoride and potassium hydroxide
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| HF | Hydrogen fluoride | 1 | Brønsted acid | Acid Weak acid |
| KOH | Potassium hydroxide | 1 | Brønsted base | Base Hydroxide base Strong base |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| KF | Potassium fluoride | 1 | Conjugate base | Salt Salt of weak acid and strong base |
| H2O | Water | 1 | Conjugate acid | Water |
Thermodynamic changes
Changes in standard condition
- Reaction of hydrogen fluoride and potassium hydroxide◆
ΔrG −122.6 kJ/mol K 3.01 × 1021 pK −21.48
| 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 | −157.2 | −122.6 | −116.2 | 30.3 |
per 1 mol of | −157.2 | −122.6 | −116.2 | 30.3 |
per 1 mol of | −157.2 | −122.6 | −116.2 | 30.3 |
per 1 mol of | −157.2 | −122.6 | −116.2 | 30.3 |
per 1 mol of | −157.2 | −122.6 | −116.2 | 30.3 |
Changes in aqueous solution (1)
- Reaction of hydrogen fluoride and potassium hydroxide◆
ΔrG −61.87 kJ/mol K 6.90 × 1010 pK −10.84
| 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 | −68.39 | −61.87 | −21.7 | – |
per 1 mol of | −68.39 | −61.87 | −21.7 | – |
per 1 mol of | −68.39 | −61.87 | −21.7 | – |
per 1 mol of | −68.39 | −61.87 | −21.7 | – |
per 1 mol of | −68.39 | −61.87 | −21.7 | – |
Changes in aqueous solution (2)
- Reaction of hydrogen fluoride and potassium hydroxide◆
ΔrG −79.90 kJ/mol K 9.95 × 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 | −55.84 | −79.90 | 80.8 | 223.9 |
per 1 mol of | −55.84 | −79.90 | 80.8 | 223.9 |
per 1 mol of | −55.84 | −79.90 | 80.8 | 223.9 |
per 1 mol of | −55.84 | −79.90 | 80.8 | 223.9 |
per 1 mol of | −55.84 | −79.90 | 80.8 | 223.9 |
Changes in aqueous solution (3)
- Reaction of hydrogen fluoride and potassium hydroxide◆
ΔrG −61.87 kJ/mol K 6.90 × 1010 pK −10.84
| 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 | −68.39 | −61.87 | −21.7 | – |
per 1 mol of | −68.39 | −61.87 | −21.7 | – |
per 1 mol of | −68.39 | −61.87 | −21.7 | – |
per 1 mol of | −68.39 | −61.87 | −21.7 | – |
per 1 mol of | −68.39 | −61.87 | −21.7 | – |
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 |
|---|---|---|---|---|
| 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] | – |
| KOH (cr) | -424.764[1] | -379.08[1] | 78.9[1] | 64.9[1] |
| KOH (g) | -231.0[1] | -232.6[1] | 238.3[1] | 49.20[1] |
| KOH (ai) | -482.37[1] | -440.50[1] | 91.6[1] | -126.8[1] |
| KOH (cr) 1 hydrate | -748.9[1] | -645.1[1] | 117.2[1] | – |
| KOH (cr) 2 hydrate | -1051.0[1] | -887.3[1] | 150.6[1] | – |
* (l):Liquid, (g):Gas, (ai):Ionized aqueous solution, (ao):Un-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 |
|---|---|---|---|---|
| KF (cr) | -567.27[1] | -537.75[1] | 66.57[1] | 49.04[1] |
| KF (g) | -325.43[1] | -343.62[1] | 226.41[1] | 35.23[1] |
| KF (ai) | -585.01[1] | -562.06[1] | 88.7[1] | -84.9[1] |
| KF (cr) 2 hydrate | -1163.621[1] | -1021.49[1] | 155.2[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, (g):Gas, (ai):Ionized aqueous solution, (l):Liquid
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°, -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
- ^ ΔfH°, -424.764 kJ · mol−1
- ^ ΔfG°, -379.08 kJ · mol−1
- ^ S°, 78.9 J · K−1 · mol−1
- ^ Cp°, 64.9 J · K−1 · mol−1
- ^ ΔfH°, -231.0 kJ · mol−1
- ^ ΔfG°, -232.6 kJ · mol−1
- ^ S°, 238.3 J · K−1 · mol−1
- ^ Cp°, 49.20 J · K−1 · mol−1
- ^ ΔfH°, -482.37 kJ · mol−1
- ^ ΔfG°, -440.50 kJ · mol−1
- ^ S°, 91.6 J · K−1 · mol−1
- ^ Cp°, -126.8 J · K−1 · mol−1
- ^ ΔfH°, -748.9 kJ · mol−1
- ^ ΔfG°, -645.1 kJ · mol−1
- ^ S°, 117.2 J · K−1 · mol−1
- ^ ΔfH°, -1051.0 kJ · mol−1
- ^ ΔfG°, -887.3 kJ · mol−1
- ^ S°, 150.6 J · K−1 · mol−1
- ^ ΔfH°, -567.27 kJ · mol−1
- ^ ΔfG°, -537.75 kJ · mol−1
- ^ S°, 66.57 J · K−1 · mol−1
- ^ Cp°, 49.04 J · K−1 · mol−1
- ^ ΔfH°, -325.43 kJ · mol−1
- ^ ΔfG°, -343.62 kJ · mol−1
- ^ S°, 226.41 J · K−1 · mol−1
- ^ Cp°, 35.23 J · K−1 · mol−1
- ^ ΔfH°, -585.01 kJ · mol−1
- ^ ΔfG°, -562.06 kJ · mol−1
- ^ S°, 88.7 J · K−1 · mol−1
- ^ Cp°, -84.9 J · K−1 · mol−1
- ^ ΔfH°, -1163.621 kJ · mol−1
- ^ ΔfG°, -1021.49 kJ · mol−1
- ^ S°, 155.2 J · K−1 · 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