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HF → H+ + F−

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Electrolytic dissociation of hydrogen fluoride
HFHydrogen fluoride
⟶
H+Hydrogen ion + F−Fluoride ion

Electrolytic dissociation of hydrogen fluoride yields hydrogen ion and fluoride ion. 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

Electrolytic dissociation of hydrogen fluoride
HFHydrogen fluoride
⟶
H+Hydrogen ion + F−Fluoride ion

General equation

Electrolytic dissociation of acid
AcidBrønsted acid
⟶
H+ + AnionConjugate base

Oxidation state of each atom

Electrolytic dissociation of hydrogen fluoride

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
HFHydrogen fluoride1
Brønsted acid
Acid

Products

Chemical formulaNameCoefficientTypeType in general
equation
H+Hydrogen ion1
–
Hydrogen ion
F−Fluoride ion1
Conjugate base
Anion

Thermodynamic changes

Changes in standard condition (1)

Electrolytic dissociation of hydrogen fluoride
◆
ΔrG18.03 kJ/mol
K0.69 × 10−3
pK3.16
HFUn-ionized aqueous solution
⟶
H+Un-ionized aqueous solution + F−Un-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
−12.5518.03−102.5–
per 1 mol of
−12.5518.03−102.5–
per 1 mol of
Hydrogen ion
−12.5518.03−102.5–
per 1 mol of
Fluoride ion
−12.5518.03−102.5–

Changes in standard condition (2)

Electrolytic dissociation of hydrogen fluoride
◆
ΔrG18.03 kJ/mol
K0.69 × 10−3
pK3.16
HFUn-ionized aqueous solution
⟶
H+Un-ionized aqueous solution + F−Un-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
−12.5518.03−102.5–
per 1 mol of
−12.5518.03−102.5–
per 1 mol of
Hydrogen ion
−12.5518.03−102.5–
per 1 mol of
Fluoride ion
−12.5518.03−102.5–

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
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]–
* (l):Liquid, (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
H+ (g)1536.202[1]–––
H+ (ao)0[1]0[1]0[1]0[1]
F− (g)-255.39[1]–––
F− (ao)-332.63[1]-278.79[1]-13.8[1]-106.7[1]
* (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)