HCl + KOH → KCl + H2O
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The reaction of hydrogen chloride and potassium hydroxide yields potassium chloride and water. This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of hydrogen chloride 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 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 chloride and potassium hydroxide
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| HCl | Hydrogen chloride | 1 | Brønsted acid | Acid Strong acid |
| KOH | Potassium hydroxide | 1 | Brønsted base | Base Hydroxide base Strong base |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| KCl | Potassium chloride | 1 | Conjugate base | Salt Salt of strong acid and strong base |
| H2O | Water | 1 | Conjugate acid | Water |
Thermodynamic changes
Changes in standard condition
- Reaction of hydrogen chloride and potassium hydroxide◆
ΔrG −171.89 kJ/mol K 1.30 × 1030 pK −30.11
| 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 | −205.506 | −171.89 | −113.3 | 32.6 |
per 1 mol of | −205.506 | −171.89 | −113.3 | 32.6 |
per 1 mol of | −205.506 | −171.89 | −113.3 | 32.6 |
per 1 mol of | −205.506 | −171.89 | −113.3 | 32.6 |
per 1 mol of | −205.506 | −171.89 | −113.3 | 32.6 |
Changes in aqueous solution
- Reaction of hydrogen chloride and potassium 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 | −55.83 | −79.89 | 80.8 | 223.9 |
per 1 mol of | −55.83 | −79.89 | 80.8 | 223.9 |
per 1 mol of | −55.83 | −79.89 | 80.8 | 223.9 |
per 1 mol of | −55.83 | −79.89 | 80.8 | 223.9 |
per 1 mol of | −55.83 | −79.89 | 80.8 | 223.9 |
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 |
|---|---|---|---|---|
| HCl (g) | -92.307[1] | -95.299[1] | 186.908[1] | 29.12[1] |
| HCl (ai) | -167.159[1] | -131.228[1] | 56.5[1] | -136.4[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] | – |
* (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 |
|---|---|---|---|---|
| KCl (cr) | -436.747[1] | -409.14[1] | 82.59[1] | 51.30[1] |
| KCl (g) | -214.14[1] | -233.0[1] | 239.10[1] | 36.48[1] |
| KCl (ai) | -419.53[1] | -414.49[1] | 159.0[1] | -114.6[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°, -92.307 kJ · mol−1
- ^ ΔfG°, -95.299 kJ · mol−1
- ^ S°, 186.908 J · K−1 · mol−1
- ^ Cp°, 29.12 J · K−1 · mol−1
- ^ ΔfH°, -167.159 kJ · mol−1
- ^ ΔfG°, -131.228 kJ · mol−1
- ^ S°, 56.5 J · K−1 · mol−1
- ^ Cp°, -136.4 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°, -436.747 kJ · mol−1
- ^ ΔfG°, -409.14 kJ · mol−1
- ^ S°, 82.59 J · K−1 · mol−1
- ^ Cp°, 51.30 J · K−1 · mol−1
- ^ ΔfH°, -214.14 kJ · mol−1
- ^ ΔfG°, -233.0 kJ · mol−1
- ^ S°, 239.10 J · K−1 · mol−1
- ^ Cp°, 36.48 J · K−1 · mol−1
- ^ ΔfH°, -419.53 kJ · mol−1
- ^ ΔfG°, -414.49 kJ · mol−1
- ^ S°, 159.0 J · K−1 · mol−1
- ^ Cp°, -114.6 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