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AlF3 + 3HCl 🔥→ AlCl3 + 3HF

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Reaction of aluminium fluoride and hydrogen chloride
AlF3Aluminium fluoride + 3HClHydrogen chloride
🔥
⟶
AlCl3Aluminium chloride + 3HFHydrogen fluoride

The reaction of aluminium fluoride and hydrogen chloride yields aluminium chloride 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

Reaction of aluminium fluoride and hydrogen chloride
AlF3Aluminium fluoride + 3HClHydrogen chloride
🔥
⟶
AlCl3Aluminium chloride + 3HFHydrogen fluoride

General equation

Reaction of salt of weak acid and strong acid with generating weak acid
Salt of weak acidBrønsted base + Strong acidBrønsted acid
⟶
Salt of strong acidConjugate base + Weak acidConjugate acid

Oxidation state of each atom

Reaction of aluminium fluoride and hydrogen chloride

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
AlF3Aluminium fluoride1
Brønsted base
Salt of weak acid
HClHydrogen chloride3
Brønsted acid
Strong acid

Products

Chemical formulaNameCoefficientTypeType in general
equation
AlCl3Aluminium chloride1
Conjugate base
Salt of strong acid
HFHydrogen fluoride3
Conjugate acid
Weak acid

Thermodynamic changes

Changes in standard condition

Reaction of aluminium fluoride and hydrogen chloride
◆
ΔrG262.5 kJ/mol
K0.10 × 10−45
pK45.99
AlF3Crystalline solid + 3HClGas
🔥
⟶
AlCl3Crystalline solid + 3HFGas
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
263.5262.54.8416.78
per 1 mol of
263.5262.54.8416.78
per 1 mol of
87.8387.501.615.593
per 1 mol of
263.5262.54.8416.78
per 1 mol of
87.8387.501.615.593

Changes in aqueous solution (1)

Reaction of aluminium fluoride and hydrogen chloride
◆
ΔrG120 kJ/mol
K0.95 × 10−21
pK21.02
AlF3Crystalline solid + 3HClIonized aqueous solution
🔥
⟶
AlCl3Ionized aqueous solution + 3HFGas
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
159120133.1–
per 1 mol of
159120133.1–
per 1 mol of
53.040.044.37–
per 1 mol of
159120133.1–
per 1 mol of
53.040.044.37–

Changes in aqueous solution (2)

Reaction of aluminium fluoride and hydrogen chloride
◆
ΔrG49 kJ/mol
K0.26 × 10−8
pK8.58
AlF3Crystalline solid + 3HClIonized aqueous solution
🔥
⟶
AlCl3Ionized aqueous solution + 3HFUn-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
1249−122.1–
per 1 mol of
1249−122.1–
per 1 mol of
4.016−40.70–
per 1 mol of
1249−122.1–
per 1 mol of
4.016−40.70–

Changes in aqueous solution (3)

Reaction of aluminium fluoride and hydrogen chloride
◆
ΔrG49 kJ/mol
K0.26 × 10−8
pK8.58
AlF3Crystalline solid + 3HClIonized aqueous solution
🔥
⟶
AlCl3Ionized aqueous solution + 3HFUn-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
1249−122.1–
per 1 mol of
1249−122.1–
per 1 mol of
4.016−40.70–
per 1 mol of
1249−122.1–
per 1 mol of
4.016−40.70–

Changes in aqueous solution (4)

Reaction of aluminium fluoride and hydrogen chloride
◆
ΔrG103 kJ/mol
K0.90 × 10−18
pK18.04
AlF3Crystalline solid + 3HClIonized aqueous solution
🔥
⟶
AlCl3Ionized aqueous solution + 3HFIonized 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
−25103−429.6–
per 1 mol of
−25103−429.6–
per 1 mol of
−8.334.3−143.2–
per 1 mol of
−25103−429.6–
per 1 mol of
−8.334.3−143.2–

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
AlF3 (cr)-1504.1[1]-1425.0[1]66.44[1]75.10[1]
AlF3 (g)-1204.6[1]-1188.2[1]277.1[1]62.63[1]
AlF3 (ai)-1531[1]-1322[1]-363.2[1]–
AlF3 (ao)-1519[1]-1414[1]-25[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, (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
AlCl3 (cr)-704.2[1]-628.8[1]110.67[1]91.84[1]
AlCl3 (g)-583.2[1]–––
AlCl3 (ai)-1033[1]-879[1]-152.3[1]–
AlCl3 (cr)
6 hydrate
-2691.6[1]-2261.1[1]318.0[1]296.2[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, (g):Gas, (ai):Ionized aqueous solution, (l):Liquid, (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)