CdCO3 + 2H2O → Cd(OH)2 + H2CO3
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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
Reaction data
Chemical equation
- Hydrolysis of cadmium carbonate
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 formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
CdCO3 | Cadmium carbonate | 1 | Brønsted base | Salt of weak acid and weak base |
H2O | Water | 2 | Brønsted acid | Water |
Products
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
Cd(OH)2 | Cadmium hydroxide | 1 | Conjugate base | Base |
H2CO3 | Carbonic acid | 1 | Conjugate acid | Acid |
Thermodynamic changes
Changes in standard condition (1)
- Hydrolysis of cadmium carbonate◆
ΔrG 78.0 kJ/mol K 0.22 × 10−13 pK 13.67
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◆
ΔrG 47.0 kJ/mol K 0.58 × 10−8 pK 8.23
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 | 61.9 | 47.0 | 51 | – |
per 1 mol of | 61.9 | 47.0 | 51 | – |
per 1 mol of | 30.9 | 23.5 | 26 | – |
per 1 mol of | 61.9 | 47.0 | 51 | – |
per 1 mol of | 61.9 | 47.0 | 51 | – |
Thermodynamic data of reactants
Chemical formula | Standard 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 formula | Standard 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
- 1Janiel J. Reed (1989)The NBS Tables of Chemical Thermodynamic Properties: Selected Values for Inorganic and C1 and C2 Organic Substances in SI UnitsNational Institute of Standards and Technology (NIST)
- ^ ΔfH°, -750.6 kJ · mol−1
- ^ ΔfG°, -669.4 kJ · mol−1
- ^ S°, 92.5 J · K−1 · mol−1
- ^ ΔfH°, -285.830 kJ · mol−1
- ^ ΔfG°, -237.129 kJ · mol−1
- ^ S°, 69.91 J · K−1 · mol−1
- ^ Cp°, 75.291 J · K−1 · mol−1
- ^ ΔfH°, -241.818 kJ · mol−1
- ^ ΔfG°, -228.572 kJ · mol−1
- ^ S°, 188.825 J · K−1 · mol−1
- ^ Cp°, 33.577 J · K−1 · mol−1
- ^ ΔfH°, -560.7 kJ · mol−1
- ^ ΔfG°, -473.6 kJ · mol−1
- ^ S°, 96. J · K−1 · mol−1
- ^ ΔfH°, -535.89 kJ · mol−1
- ^ ΔfG°, -392.10 kJ · mol−1
- ^ S°, -94.6 J · K−1 · mol−1
- ^ ΔfG°, -442.6 kJ · mol−1
- ^ ΔfH°, -699.65 kJ · mol−1
- ^ ΔfG°, -623.08 kJ · mol−1
- ^ S°, 187.4 J · K−1 · mol−1