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ZnSO4 + Na2S 💧→ ZnS↓ + Na2SO4

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Reaction of zinc sulfate and sodium sulfide
ZnSO4Zinc sulfate + Na2SSodium sulfide
💧
⟶
ZnS↓Zinc sulfide + Na2SO4Sodium sulfate

The reaction of zinc sulfate and sodium sulfide yields zinc sulfide and sodium 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 sodium sulfide
ZnSO4Zinc sulfate + Na2SSodium sulfide
💧
⟶
ZnS↓Zinc sulfide + Na2SO4Sodium 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 sodium sulfide

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
ZnSO4Zinc sulfate1
Lewis acid
Very soluble in water
Na2SSodium sulfide1
Lewis base
Soluble in water

Products

Chemical formulaNameCoefficientTypeType in general
equation
ZnSZinc sulfide1
Lewis conjugate
Insoluble in water
Na2SO4Sodium sulfate1
Non-redox product
–

Thermodynamic changes

Changes in standard condition (1)

Reaction of zinc sulfate and sodium sulfide
◆
ΔrG−250.2 kJ/mol
K6.81 × 1043
pK−43.83
ZnSO4Crystalline solid + Na2SCrystalline solid
💧
⟶
ZnS↓Crystalline solid + Na2SO4Crystalline solidorthorhombic
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
−245.5−250.213.1–
per 1 mol of
−245.5−250.213.1–
per 1 mol of
−245.5−250.213.1–
per 1 mol of
−245.5−250.213.1–
per 1 mol of
−245.5−250.213.1–

Changes in standard condition (2)

Reaction of zinc sulfate and sodium sulfide
ZnSO4Crystalline solid + Na2SCrystalline solid
💧
⟶
ZnS↓Crystalline solid + Na2SO4Crystalline solidmetastable
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
––18.4–
per 1 mol of
––18.4–
per 1 mol of
––18.4–
per 1 mol of
––18.4–
per 1 mol of
––18.4–

Changes in aqueous solution (1)

Reaction of zinc sulfate and sodium sulfide
◆
ΔrG−126.7 kJ/mol
K1.57 × 1022
pK−22.20
ZnSO4Un-ionized aqueous solution + Na2SIonized aqueous solution
💧
⟶
ZnS↓Crystalline solid + Na2SO4Ionized 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
−100.5−126.787.5–
per 1 mol of
−100.5−126.787.5–
per 1 mol of
−100.5−126.787.5–
per 1 mol of
−100.5−126.787.5–
per 1 mol of
−100.5−126.787.5–

Changes in aqueous solution (2)

Reaction of zinc sulfate and sodium sulfide
◆
ΔrG−140.0 kJ/mol
K3.36 × 1024
pK−24.53
ZnSO4Ionized aqueous solution + Na2SIonized aqueous solution
💧
⟶
ZnS↓Crystalline solid + Na2SO4Ionized 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
−85.0−140.0184.5–
per 1 mol of
−85.0−140.0184.5–
per 1 mol of
−85.0−140.0184.5–
per 1 mol of
−85.0−140.0184.5–
per 1 mol of
−85.0−140.0184.5–

Changes in aqueous solution (3)

Reaction of zinc sulfate and sodium sulfide
◆
ΔrG−126.7 kJ/mol
K1.57 × 1022
pK−22.20
ZnSO4Un-ionized aqueous solution + Na2SIonized aqueous solution
💧
⟶
ZnS↓Crystalline solid + Na2SO4Ionized 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
−100.5−126.787.5–
per 1 mol of
−100.5−126.787.5–
per 1 mol of
−100.5−126.787.5–
per 1 mol of
−100.5−126.787.5–
per 1 mol of
−100.5−126.787.5–

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
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]
Na2S (cr)-364.8[1]-349.8[1]83.7[1]–
Na2S (ai)-447.3[1]-438.1[1]103.3[1]–
Na2S (cr)
4.5 hydrate
-1725.9[1]–––
Na2S (cr)
5 hydrate
-1886.6[1]–––
Na2S (cr)
9 hydrate
-3074.0[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
ZnS (cr)-205.98[1]-201.29[1]57.7[1]46.0[1]
Na2SO4 (cr)
orthorhombic
-1387.08[1]-1270.16[1]149.58[1]128.20[1]
Na2SO4 (cr)
metastable
––154.934[1]129.29[1]
Na2SO4 (ai)-1389.51[1]-1268.36[1]138.1[1]-201[1]
Na2SO4 (cr)
10 hydrate
-4327.26[1]-3646.85[1]592.0[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)