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KF + HIO3 → KIO3 + HF↑

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
  1. 1Reaction data
  2. 2Thermodynamic changes
  3. 3References
  4. 4Related categories

Reaction data

Chemical equation

General equation

Oxidation state of each atom

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
KFPotassium fluoride1
Brønsted base
Salt of weak acid
Salt of volatile acid
HIO3Iodic acid1
Brønsted acid
Strong acid
Nonvolatile acid

Products

Chemical formulaNameCoefficientTypeType in general
equation
KIO3Potassium iodate1
Conjugate base
Salt of strong acid
Salt of non volatile acid
HFHydrogen fluoride1
Conjugate acid
Weak acid
Volatile acid

Thermodynamic changes

Changes in standard condition

Reaction of potassium fluoride and iodic acid
KFCrystalline solid + HIO3Crystalline solid
KIO3Crystalline solid + HFGas
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
ΔrG10.3 kJ/mol
K0.16 × 10−1
pK1.80
KFIonized aqueous solution + HIO3Un-ionized aqueous solution
KIO3Ionized aqueous solution + HFGas
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
51.610.3139.1
per 1 mol of
51.610.3139.1
per 1 mol of
51.610.3139.1
per 1 mol of
51.610.3139.1
per 1 mol of
51.610.3139.1

Changes in aqueous solution (2)

Reaction of potassium fluoride and iodic acid
ΔrG−13.4 kJ/mol
K2.23 × 102
pK−2.35
KFIonized aqueous solution + HIO3Un-ionized aqueous solution
KIO3Ionized aqueous solution + HFUn-ionized aqueous solution
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
2.6−13.454.0
per 1 mol of
2.6−13.454.0
per 1 mol of
2.6−13.454.0
per 1 mol of
2.6−13.454.0
per 1 mol of
2.6−13.454.0

Changes in aqueous solution (3)

Reaction of potassium fluoride and iodic acid
ΔrG−13.4 kJ/mol
K2.23 × 102
pK−2.35
KFIonized aqueous solution + HIO3Un-ionized aqueous solution
KIO3Ionized aqueous solution + HFUn-ionized aqueous solution
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
2.6−13.454.0
per 1 mol of
2.6−13.454.0
per 1 mol of
2.6−13.454.0
per 1 mol of
2.6−13.454.0
per 1 mol of
2.6−13.454.0

Changes in aqueous solution (4)

Reaction of potassium fluoride and iodic acid
ΔrG4.7 kJ/mol
K0.15 × 100
pK0.82
KFIonized aqueous solution + HIO3Un-ionized aqueous solution
KIO3Ionized aqueous solution + HFIonized aqueous solution
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
−9.94.7−48.5
per 1 mol of
−9.94.7−48.5
per 1 mol of
−9.94.7−48.5
per 1 mol of
−9.94.7−48.5
per 1 mol of
−9.94.7−48.5

Thermodynamic data of reactants

Chemical formulaStandard 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 formulaStandard 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

  1. 1
    Janiel J. Reed (1989)
    The NBS Tables of Chemical Thermodynamic Properties: Selected Values for Inorganic and C1 and C2 Organic Substances in SI Units
    National Institute of Standards and Technology (NIST)