KCl + HIO3 🔥→ KIO3 + HCl↑
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- Reaction of potassium chloride and iodic acid
The reaction of potassium chloride and iodic acid yields potassium iodate and hydrogen chloride. This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of potassium chloride and iodic acid
General equation
- Salt of volatile acidBrønsted base + Nonvolatile acidBrønsted acid ⟶ Salt of non volatile acidConjugate base + Volatile acidConjugate acid
Oxidation state of each atom
- Reaction of potassium chloride and iodic acid
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| KCl | Potassium chloride | 1 | Brønsted base | Salt of volatile acid |
| HIO3 | Iodic acid | 1 | Brønsted acid | Nonvolatile acid |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| KIO3 | Potassium iodate | 1 | Conjugate base | Salt of non volatile acid |
| HCl | Hydrogen chloride | 1 | Conjugate acid | Volatile acid |
Thermodynamic changes
Changes in standard condition
- Reaction of potassium chloride and iodic acid
| 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 | 73.2 | – | – | – |
per 1 mol of | 73.2 | – | – | – |
per 1 mol of | 73.2 | – | – | – |
per 1 mol of | 73.2 | – | – | – |
per 1 mol of | 73.2 | – | – | – |
Changes in aqueous solution (1)
- Reaction of potassium chloride and iodic acid◆
ΔrG 40.6 kJ/mol K 0.77 × 10−7 pK 7.11
| 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 | 64.9 | 40.6 | 81.9 | – |
per 1 mol of | 64.9 | 40.6 | 81.9 | – |
per 1 mol of | 64.9 | 40.6 | 81.9 | – |
per 1 mol of | 64.9 | 40.6 | 81.9 | – |
per 1 mol of | 64.9 | 40.6 | 81.9 | – |
Changes in aqueous solution (2)
- Reaction of potassium chloride and iodic acid◆
ΔrG 4.7 kJ/mol K 0.15 × 100 pK 0.82
| 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 | −9.9 | 4.7 | −48.5 | – |
per 1 mol of | −9.9 | 4.7 | −48.5 | – |
per 1 mol of | −9.9 | 4.7 | −48.5 | – |
per 1 mol of | −9.9 | 4.7 | −48.5 | – |
per 1 mol of | −9.9 | 4.7 | −48.5 | – |
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 |
|---|---|---|---|---|
| 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] |
| HIO3 (cr) | -230.1[1] | – | – | – |
| HIO3 (ao) | -211.3[1] | -132.6[1] | 166.9[1] | – |
* (cr):Crystalline solid, (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 |
|---|---|---|---|---|
| KIO3 (cr) | -501.37[1] | -418.35[1] | 151.46[1] | 106.48[1] |
| KIO3 (ai) | -473.6[1] | -411.2[1] | 220.9[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] |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (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°, -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°, -230.1 kJ · mol−1
- ^ ΔfH°, -211.3 kJ · mol−1
- ^ ΔfG°, -132.6 kJ · mol−1
- ^ S°, 166.9 J · K−1 · mol−1
- ^ ΔfH°, -501.37 kJ · mol−1
- ^ ΔfG°, -418.35 kJ · mol−1
- ^ S°, 151.46 J · K−1 · mol−1
- ^ Cp°, 106.48 J · K−1 · mol−1
- ^ ΔfH°, -473.6 kJ · mol−1
- ^ ΔfG°, -411.2 kJ · mol−1
- ^ S°, 220.9 J · K−1 · mol−1
- ^ 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