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2KF + Na2CrO4 💧→ K2CrO4↓ + 2NaF

The reaction of potassium fluoride and sodium chromate yields potassium chromate and sodium 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 fluoride2
Lewis acid
Very soluble in water
Na2CrO4Sodium chromate1
Lewis base
Very soluble in water

Products

Chemical formulaNameCoefficientTypeType in general
equation
K2CrO4Potassium chromate1
Lewis conjugate
Insoluble in water
NaFSodium fluoride2
Non-redox product

Thermodynamic changes

Changes in standard condition

Reaction of potassium fluoride and sodium chromate
ΔrG−72.3 kJ/mol
K4.64 × 1012
pK−12.67
2KFCrystalline solid + Na2CrO4Crystalline solid
💧
K2CrO4Crystalline solid + 2NaFCrystalline solid
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
−74.3−72.3−6.71−0.51
per 1 mol of
−37.1−36.1−3.35−0.255
per 1 mol of
−74.3−72.3−6.71−0.510
per 1 mol of
−74.3−72.3−6.71−0.510
per 1 mol of
−37.1−36.1−3.35−0.255

Changes in aqueous solution

Reaction of potassium fluoride and sodium chromate
ΔrG0.04 kJ/mol
K0.98 × 100
pK0.01
2KFIonized aqueous solution + Na2CrO4Ionized aqueous solution
💧
K2CrO4Ionized aqueous solution + 2NaFIonized 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
0.000.040.0
per 1 mol of
0.000.02000.0
per 1 mol of
0.000.04000.0
per 1 mol of
0.000.04000.0
per 1 mol of
0.000.02000.0

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]
Na2CrO4 (cr)-1342.2[1]-1234.93[1]176.61[1]142.13[1]
Na2CrO4 (ai)-1361.39[1]-1251.58[1]168.2[1]
Na2CrO4 (cr)
4 hydrate
-2528.8[1]
Na2CrO4 (cr)
10 hydrate
-4281.1[1]
* (cr):Crystalline solid, (g):Gas, (ai):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
K2CrO4 (cr)-1403.7[1]-1295.7[1]200.12[1]145.98[1]
K2CrO4 (ai)-1385.91[1]-1294.30[1]255.2[1]
NaF (cr)-573.647[1]-543.494[1]51.46[1]46.86[1]
NaF (g)-291.2[1]-310.5[1]217.59[1]34.221[1]
NaF (ai)-572.75[1]-540.68[1]45.2[1]-60.2[1]
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (g):Gas

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)