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K2O + 2HF → 2KF + H2O

The reaction of potassium oxide and hydrogen fluoride yields potassium fluoride and water. 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

Reaction of basic oxide and acid
Basic oxideBrønsted base + AcidBrønsted acid
SaltConjugate base + H2OConjugate acid

Oxidation state of each atom

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
K2OPotassium oxide1
Brønsted base
Basic oxide
Strongly basic oxide
HFHydrogen fluoride2
Brønsted acid
Acid
Weak acid

Products

Chemical formulaNameCoefficientTypeType in general
equation
KFPotassium fluoride2
Conjugate base
Salt
Salt of weak acid and strong base
H2OWater1
Conjugate acid
Water

Thermodynamic changes

Changes in standard condition

Reaction of potassium oxide and hydrogen fluoride
ΔrG−444.1 kJ/mol
K6.35 × 1077
pK−77.80
K2OCrystalline solid + 2HFGas
2KFCrystalline solid + H2OLiquid
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
−516.7−444.1−238.631.4
per 1 mol of
−516.7−444.1−238.631.4
per 1 mol of
−258.4−222.1−119.315.7
per 1 mol of
−258.4−222.1−119.315.7
per 1 mol of
−516.7−444.1−238.631.4

Changes in aqueous solution (1)

Reaction of potassium oxide and hydrogen fluoride
ΔrG−445.5 kJ/mol
K1.12 × 1078
pK−78.05
K2OCrystalline solid + 2HFUn-ionized aqueous solution
2KFIonized aqueous solution + H2OLiquid
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
−454.2−445.5−24.2
per 1 mol of
−454.2−445.5−24.2
per 1 mol of
−227.1−222.8−12.1
per 1 mol of
−227.1−222.8−12.1
per 1 mol of
−454.2−445.5−24.2

Changes in aqueous solution (2)

Reaction of potassium oxide and hydrogen fluoride
ΔrG−481.6 kJ/mol
K2.36 × 1084
pK−84.37
K2OCrystalline solid + 2HFIonized aqueous solution
2KFIonized aqueous solution + H2OLiquid
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
−429.1−481.6180.835.2
per 1 mol of
−429.1−481.6180.835.2
per 1 mol of
−214.6−240.890.4017.6
per 1 mol of
−214.6−240.890.4017.6
per 1 mol of
−429.1−481.6180.835.2

Changes in aqueous solution (3)

Reaction of potassium oxide and hydrogen fluoride
ΔrG−445.5 kJ/mol
K1.12 × 1078
pK−78.05
K2OCrystalline solid + 2HFUn-ionized aqueous solution
2KFIonized aqueous solution + H2OLiquid
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
−454.2−445.5−24.2
per 1 mol of
−454.2−445.5−24.2
per 1 mol of
−227.1−222.8−12.1
per 1 mol of
−227.1−222.8−12.1
per 1 mol of
−454.2−445.5−24.2

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
K2O (cr)-361.5[1]-322.1[2]94.1[2]83.7[2]
K2O (g)-63[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, (l):Liquid, (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
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]
H2O (cr)
H2O (l)-285.830[1]-237.129[1]69.91[1]75.291[1]
H2O (g)-241.818[1]-228.572[1]188.825[1]33.577[1]
* (cr):Crystalline solid, (g):Gas, (ai):Ionized aqueous solution, (l):Liquid

References

List of references

  1. 1
  2. 2
    James G. Speight (2017)
    Lange's Handbook of Chemistry, 17th edition
    McGraw Hill Education