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Fe2(SO4)3 + 3Sr(OH)2 → 3SrSO4↓ + 2Fe(OH)3

The reaction of iron(III) sulfate and strontium hydroxide yields strontium sulfate and iron(III) hydroxide. 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
Fe2(SO4)3Iron(III) sulfate1
Brønsted acid
Lewis acid
Salt of weak base
Soluble in water
Sr(OH)2Strontium hydroxide3
Brønsted base
Lewis base
Strong base
Soluble in water

Products

Chemical formulaNameCoefficientTypeType in general
equation
SrSO4Strontium sulfate3
Conjugate acid
Lewis conjugate
Salt of strong base
Very slightly soluble in water
Fe(OH)3Iron(III) hydroxide2
Conjugate base
Lewis conjugate
Weak base
Insoluble in water

Thermodynamic changes

Changes in standard condition (1)

Reaction of iron(III) sulfate and strontium hydroxide
Fe2(SO4)3Crystalline solid + 3Sr(OH)2Crystalline solid
3SrSO4Crystalline solid + 2Fe(OH)3Crystalline solidprecipitated
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
−546.8
per 1 mol of
−546.8
−182.3
per 1 mol of
−182.3
−273.4

Changes in standard condition (2)

Reaction of iron(III) sulfate and strontium hydroxide
Fe2(SO4)3Crystalline solid + 3Sr(OH)2Crystalline solid
3SrSO4Crystalline solidprecipitated + 2Fe(OH)3Crystalline solidprecipitated
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
−536.9
per 1 mol of
−536.9
−179.0
per 1 mol of
−179.0
−268.4

Changes in aqueous solution (1)

Reaction of iron(III) sulfate and strontium hydroxide
Fe2(SO4)3Ionized aqueous solution + 3Sr(OH)2Crystalline solid
3SrSO4Crystalline solid + 2Fe(OH)3Un-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
per 1 mol of
per 1 mol of

Changes in aqueous solution (2)

Reaction of iron(III) sulfate and strontium hydroxide
Fe2(SO4)3Ionized aqueous solution + 3Sr(OH)2Crystalline solid
3SrSO4Crystalline solidprecipitated + 2Fe(OH)3Un-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
per 1 mol of
per 1 mol of

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
Fe2(SO4)3 (cr)-2581.5[1]
Fe2(SO4)3 (ai)-2825.0[1]-2242.8[1]-571.5[1]
Sr(OH)2 (cr)-959.0[1]
Sr(OH)2 (g)-565[1]
Sr(OH)2 (cr)
1 hydrate
-1264.8[1]
Sr(OH)2 (cr)
8 hydrate
-3352.2[1]
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (g):Gas

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
SrSO4 (cr)-1453.1[1]-1340.9[1]117[1]
SrSO4 (cr)
precipitated
-1449.8[1]
SrSO4 (ai)-1455.07[1]-1304.00[1]-12.6[1]
Fe(OH)3 (cr)
precipitated
-823.0[1]-696.5[1]106.7[1]
Fe(OH)3 (ao)-659.3[1]
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution

References

List of references

  1. 1