KF + HIO3 → KIO3 + HF↑
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The reaction of potassium fluoride and iodic acid yields potassium iodate and hydrogen fluoride. This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of potassium fluoride and iodic acid
General equation
- Salt of weak acidBrønsted base + Strong acidBrønsted acid ⟶ Salt of strong acidConjugate base + Weak acidConjugate acid
- 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 fluoride and iodic acid
Reactants
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
KF | Potassium fluoride | 1 | Brønsted base | Salt of weak acid Salt of volatile acid |
HIO3 | Iodic acid | 1 | Brønsted acid | Strong acid Nonvolatile acid |
Products
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
KIO3 | Potassium iodate | 1 | Conjugate base | Salt of strong acid Salt of non volatile acid |
HF | Hydrogen fluoride | 1 | Conjugate acid | Weak acid Volatile acid |
Thermodynamic changes
Changes in standard condition
- Reaction of potassium fluoride 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 | 24.9 | – | – | – |
per 1 mol of | 24.9 | – | – | – |
per 1 mol of | 24.9 | – | – | – |
per 1 mol of | 24.9 | – | – | – |
per 1 mol of | 24.9 | – | – | – |
Changes in aqueous solution (1)
- Reaction of potassium fluoride and iodic acid◆
ΔrG 10.3 kJ/mol K 0.16 × 10−1 pK 1.80
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 | 51.6 | 10.3 | 139.1 | – |
per 1 mol of | 51.6 | 10.3 | 139.1 | – |
per 1 mol of | 51.6 | 10.3 | 139.1 | – |
per 1 mol of | 51.6 | 10.3 | 139.1 | – |
per 1 mol of | 51.6 | 10.3 | 139.1 | – |
Changes in aqueous solution (2)
- Reaction of potassium fluoride and iodic acid◆
ΔrG −13.4 kJ/mol K 2.23 × 102 pK −2.35
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 | 2.6 | −13.4 | 54.0 | – |
per 1 mol of | 2.6 | −13.4 | 54.0 | – |
per 1 mol of | 2.6 | −13.4 | 54.0 | – |
per 1 mol of | 2.6 | −13.4 | 54.0 | – |
per 1 mol of | 2.6 | −13.4 | 54.0 | – |
Changes in aqueous solution (3)
- Reaction of potassium fluoride and iodic acid◆
ΔrG −13.4 kJ/mol K 2.23 × 102 pK −2.35
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 | 2.6 | −13.4 | 54.0 | – |
per 1 mol of | 2.6 | −13.4 | 54.0 | – |
per 1 mol of | 2.6 | −13.4 | 54.0 | – |
per 1 mol of | 2.6 | −13.4 | 54.0 | – |
per 1 mol of | 2.6 | −13.4 | 54.0 | – |
Changes in aqueous solution (4)
- Reaction of potassium fluoride 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 |
---|---|---|---|---|
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] | – |
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] | – |
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°, -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°, -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°, -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