SrSO4 → Sr2+ + SO42−
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- Electrolytic dissociation of strontium sulfate
Electrolytic dissociation of strontium sulfate yields strontium ion and sulfate ion. This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Electrolytic dissociation of strontium sulfate
General equation
- Electrolytic dissociation of salt
- SaltLewis conjugate ⟶ CationLewis acid + AnionLewis base
Oxidation state of each atom
- Electrolytic dissociation of strontium sulfate
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| SrSO4 | Strontium sulfate | 1 | Lewis conjugate | Salt |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Sr2+ | Strontium ion | 1 | Lewis acid | Cation |
| SO42− | Sulfate ion | 1 | Lewis base | Anion |
Thermodynamic changes
Changes in standard condition (1)
- Electrolytic dissociation of strontium sulfate◆
ΔrG 36.9 kJ/mol K 0.34 × 10−6 pK 6.46
| 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 | −2.0 | 36.9 | −130 | – |
per 1 mol of | −2.0 | 36.9 | −130 | – |
per 1 mol of Strontium ion | −2.0 | 36.9 | −130 | – |
per 1 mol of Sulfate ion | −2.0 | 36.9 | −130 | – |
Changes in standard condition (2)
- Electrolytic dissociation of strontium sulfate
- SrSO4Crystalline solidprecipitatedSr2+Un-ionized aqueous solution + SO42−Un-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 | −5.3 | – | – | – |
per 1 mol of | −5.3 | – | – | – |
per 1 mol of Strontium ion | −5.3 | – | – | – |
per 1 mol of Sulfate ion | −5.3 | – | – | – |
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 |
|---|---|---|---|---|
| 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] | – |
* (cr):Crystalline solid, (ai):Ionized aqueous solution
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 |
|---|---|---|---|---|
| Sr2+ (g) | 1790.54[1] | – | – | – |
| Sr2+ (ao) | -545.80[1] | -559.48[1] | -32.6[1] | – |
| SO42− (ao) | -909.27[1] | -744.53[1] | 20.1[1] | -293[1] |
* (g):Gas, (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°, -1453.1 kJ · mol−1
- ^ ΔfG°, -1340.9 kJ · mol−1
- ^ S°, 117. J · K−1 · mol−1
- ^ ΔfH°, -1449.8 kJ · mol−1
- ^ ΔfH°, -1455.07 kJ · mol−1
- ^ ΔfG°, -1304.00 kJ · mol−1
- ^ S°, -12.6 J · K−1 · mol−1
- ^ ΔfH°, 1790.54 kJ · mol−1
- ^ ΔfH°, -545.80 kJ · mol−1
- ^ ΔfG°, -559.48 kJ · mol−1
- ^ S°, -32.6 J · K−1 · mol−1
- ^ ΔfH°, -909.27 kJ · mol−1
- ^ ΔfG°, -744.53 kJ · mol−1
- ^ S°, 20.1 J · K−1 · mol−1
- ^ Cp°, -293. J · K−1 · mol−1