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CdCO3 + 2H2O → Cd(OH)2 + H2CO3

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Hydrolysis of cadmium carbonate
CdCO3Cadmium carbonate + 2H2OWater
⟶
Cd(OH)2Cadmium hydroxide + H2CO3Carbonic acid

The reaction of cadmium carbonate and water yields cadmium hydroxide and carbonic acid. 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

Hydrolysis of cadmium carbonate
CdCO3Cadmium carbonate + 2H2OWater
⟶
Cd(OH)2Cadmium hydroxide + H2CO3Carbonic acid

General equation

Hydrolysis of salt
Salt of weak acid and weak baseBrønsted base + H2OBrønsted acid
⟶
Base/Basic saltConjugate base + Acid/Acid salt/HydrideConjugate acid

Oxidation state of each atom

Hydrolysis of cadmium carbonate

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
CdCO3Cadmium carbonate1
Brønsted base
Salt of weak acid and weak base
H2OWater2
Brønsted acid
Water

Products

Chemical formulaNameCoefficientTypeType in general
equation
Cd(OH)2Cadmium hydroxide1
Conjugate base
Base
H2CO3Carbonic acid1
Conjugate acid
Acid

Thermodynamic changes

Changes in standard condition (1)

Hydrolysis of cadmium carbonate
◆
ΔrG78.0 kJ/mol
K0.22 × 10−13
pK13.67
CdCO3Crystalline solid + 2H2OLiquid
⟶
Cd(OH)2Un-ionized aqueous solution + H2CO3Un-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
–78.0––
per 1 mol of
–78.0––
per 1 mol of
–39.0––
per 1 mol of
–78.0––
per 1 mol of
–78.0––

Changes in standard condition (2)

Hydrolysis of cadmium carbonate
◆
ΔrG47.0 kJ/mol
K0.58 × 10−8
pK8.23
CdCO3Crystalline solid + 2H2OLiquid
⟶
Cd(OH)2Crystalline solidprecipitated + H2CO3Un-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
61.947.051–
per 1 mol of
61.947.051–
per 1 mol of
30.923.526–
per 1 mol of
61.947.051–
per 1 mol of
61.947.051–

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
CdCO3 (cr)-750.6[1]-669.4[1]92.5[1]–
H2O (cr)––––
H2O (l)-285.830[1]-237.129[1]69.91[1]75.291[1]
H2O (g)-241.818[1]-228.572[1]188.825[1]33.577[1]
* (cr):Crystalline solid, (l):Liquid, (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
Cd(OH)2 (cr)
precipitated
-560.7[1]-473.6[1]96[1]–
Cd(OH)2 (ai)-535.89[1]-392.10[1]-94.6[1]–
Cd(OH)2 (ao)–-442.6[1]––
H2CO3 (ao)-699.65[1]-623.08[1]187.4[1]–
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (ao):Un-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)