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HgCl2 + CdSO4 💧→ HgSO4↓ + CdCl2

The reaction of mercury(II) chloride and cadmium sulfate yields mercury(II) sulfate and cadmium chloride. 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
HgCl2Mercury(II) chloride1
Lewis acid
Soluble in water
CdSO4Cadmium sulfate1
Lewis base
Very soluble in water

Products

Chemical formulaNameCoefficientTypeType in general
equation
HgSO4Mercury(II) sulfate1
Lewis conjugate
Very slightly soluble in water
CdCl2Cadmium chloride1
Non-redox product

Thermodynamic changes

Changes in standard condition

Reaction of mercury(II) chloride and cadmium sulfate
HgCl2Crystalline solid + CdSO4Crystalline solid
💧
HgSO4Crystalline solid + CdCl2Crystalline 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
58.6
58.6
per 1 mol of
58.6
58.6
per 1 mol of
58.6

Changes in aqueous solution (1)

Reaction of mercury(II) chloride and cadmium sulfate
ΔrG67.7 kJ/mol
K0.14 × 10−11
pK11.86
HgCl2Un-ionized aqueous solution + CdSO4Crystalline solid
💧
HgSO4Un-ionized aqueous solution + CdCl2Ionized 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
67.7
67.7
per 1 mol of
67.7
67.7
per 1 mol of
67.7

Changes in aqueous solution (2)

Reaction of mercury(II) chloride and cadmium sulfate
ΔrG48.4 kJ/mol
K0.33 × 10−8
pK8.48
HgCl2Un-ionized aqueous solution + CdSO4Crystalline solid
💧
HgSO4Un-ionized aqueous solution + CdCl2Un-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
48.4
48.4
per 1 mol of
48.4
48.4
per 1 mol of
48.4

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
HgCl2 (cr)-224.3[1]-178.6[1]146.0[1]
HgCl2 (ao)-216.3[1]-173.2[1]155[1]
CdSO4 (cr)-933.28[1]-822.72[1]123.039[1]99.58[1]
CdSO4 (ai)-985.16[1]-822.13[1]-53.1[1]
CdSO4 (cr)
1 hydrate
-1239.55[1]-1068.73[1]154.030[1]134.56[1]
CdSO4 (cr)
8/3 hydrate
-1729.4[1]-1465.141[1]229.630[1]213.26[1]
* (cr):Crystalline solid, (ao):Un-ionized aqueous solution, (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
HgSO4 (cr)-707.5[1]
HgSO4 (ao)-588.2[1]
CdCl2 (cr)-391.50[1]-343.93[1]115.27[1]74.68[1]
CdCl2 (ai)-410.20[1]-340.068[1]39.7[1]
CdCl2 (ao)-405.0[1]-359.29[1]121.8[1]
CdCl2 (cr)
1 hydrate
-688.44[1]-586.975[1]167.8[1]
CdCl2 (cr)
2.5 hydrate
-1131.94[1]-943.939[1]227.2[1]
* (cr):Crystalline solid, (ao):Un-ionized aqueous solution, (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)