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ZnSO4 + 2NH4F 💧→ ZnF2↓ + (NH4)2SO4

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Reaction of zinc sulfate and ammonium fluoride
ZnSO4Zinc sulfate + 2NH4FAmmonium fluoride
💧
⟶
ZnF2↓Zinc fluoride + (NH4)2SO4Ammonium sulfate

The reaction of zinc sulfate and ammonium fluoride yields zinc fluoride and ammonium sulfate. 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 zinc sulfate and ammonium fluoride
ZnSO4Zinc sulfate + 2NH4FAmmonium fluoride
💧
⟶
ZnF2↓Zinc fluoride + (NH4)2SO4Ammonium sulfate

General equation

Precipitation reaction
Miscible with water/Very soluble in water/Soluble in waterLewis acid + Miscible with water/Very soluble in water/Soluble in waterLewis base
💧
⟶
Insoluble in water/Very slightly soluble in water/Slightly soluble in waterLewis conjugate + Product(Non-redox product)

Oxidation state of each atom

Reaction of zinc sulfate and ammonium fluoride

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
ZnSO4Zinc sulfate1
Lewis acid
Very soluble in water
NH4FAmmonium fluoride2
Lewis base
Very soluble in water

Products

Chemical formulaNameCoefficientTypeType in general
equation
ZnF2Zinc fluoride1
Lewis conjugate
Slightly soluble in water
(NH4)2SO4Ammonium sulfate1
Non-redox product
–

Thermodynamic changes

Changes in standard condition

Reaction of zinc sulfate and ammonium fluoride
◆
ΔrG−46.1 kJ/mol
K1.19 × 108
pK−8.08
ZnSO4Crystalline solid + 2NH4FCrystalline solid
💧
⟶
ZnF2↓Crystalline solid + (NH4)2SO4Crystalline 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
−34.5−46.139.423.4
per 1 mol of
−34.5−46.139.423.4
per 1 mol of
−17.3−23.119.711.7
per 1 mol of
−34.5−46.139.423.4
per 1 mol of
−34.5−46.139.423.4

Changes in aqueous solution (1)

Reaction of zinc sulfate and ammonium fluoride
◆
ΔrG4.6 kJ/mol
K0.16 × 100
pK0.81
ZnSO4Un-ionized aqueous solution + 2NH4FIonized aqueous solution
💧
⟶
ZnF2↓Crystalline solid + (NH4)2SO4Ionized 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
39.34.6116.4–
per 1 mol of
39.34.6116.4–
per 1 mol of
19.62.358.20–
per 1 mol of
39.34.6116.4–
per 1 mol of
39.34.6116.4–

Changes in aqueous solution (2)

Reaction of zinc sulfate and ammonium fluoride
◆
ΔrG−8.7 kJ/mol
K3.34 × 101
pK−1.52
ZnSO4Ionized aqueous solution + 2NH4FIonized aqueous solution
💧
⟶
ZnF2↓Crystalline solid + (NH4)2SO4Ionized 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
54.8−8.7213.4233
per 1 mol of
54.8−8.7213.4233
per 1 mol of
27.4−4.3106.7117
per 1 mol of
54.8−8.7213.4233
per 1 mol of
54.8−8.7213.4233

Changes in aqueous solution (3)

Reaction of zinc sulfate and ammonium fluoride
◆
ΔrG4.6 kJ/mol
K0.16 × 100
pK0.81
ZnSO4Un-ionized aqueous solution + 2NH4FIonized aqueous solution
💧
⟶
ZnF2↓Crystalline solid + (NH4)2SO4Ionized 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
39.34.6116.4–
per 1 mol of
39.34.6116.4–
per 1 mol of
19.62.358.20–
per 1 mol of
39.34.6116.4–
per 1 mol of
39.34.6116.4–

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
ZnSO4 (cr)-982.8[1]-871.5[1]110.5[1]99.2[1]
ZnSO4 (ai)-1063.15[1]-891.59[1]-92.0[1]-247[1]
ZnSO4 (ao)-1047.7[1]-904.9[1]5.0[1]–
ZnSO4 (cr)
1 hydrate
-1304.49[1]-1131.99[1]138.5[1]–
ZnSO4 (cr)
6 hydrate
-2777.46[1]-2324.44[1]363.6[1]357.69[1]
ZnSO4 (cr)
7 hydrate
-3077.75[1]-2562.67[1]388.7[1]383.42[1]
NH4F (cr)-463.96[1]-348.68[1]71.96[1]65.27[1]
NH4F (ai)-465.14[1]-358.09[1]99.6[1]-26.8[1]
* (cr):Crystalline solid, (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
ZnF2 (cr)-764.4[1]-713.3[1]73.68[1]65.65[1]
ZnF2 (ai)-819.14[1]-704.64[1]-139.7[1]-167[1]
(NH4)2SO4 (cr)-1180.85[1]-901.67[1]220.1[1]187.49[1]
(NH4)2SO4 (ai)-1174.28[1]-903.14[1]246.9[1]-133.1[1]
* (cr):Crystalline solid, (ai):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)