K+ + SO42− → KSO4−
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- Reaction of potassium ion and sulfate ion
- K+Potassium ion + SO42−Sulfate ionKSO4−Potassium sulfate ion⟶
The reaction of potassium ion and sulfate ion yields potassium sulfate ion (Other reactions are here). This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of potassium ion and sulfate ion
- K+Potassium ion + SO42−Sulfate ionKSO4−Potassium sulfate ion⟶
General equation
- Reaction of cation and anion
- CationLewis acid + AnionLewis base ⟶ ProductLewis conjugate + (H2O)
Oxidation state of each atom
- Reaction of potassium ion and sulfate ion
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| K+ | Potassium ion | 1 | Lewis acid | Cation |
| SO42− | Sulfate ion | 1 | Lewis base | Anion |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| KSO4− | Potassium sulfate ion | 1 | Lewis conjugate | – |
Thermodynamic changes
Changes in standard condition
- Reaction of potassium ion and sulfate ion◆
ΔrG −4.27 kJ/mol K 5.60 × 100 pK −0.75 - K+Un-ionized aqueous solution + SO42−Un-ionized aqueous solutionKSO4−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 | 4.23 | −4.27 | 28.4 | – |
per 1 mol of Potassium ion | 4.23 | −4.27 | 28.4 | – |
per 1 mol of Sulfate ion | 4.23 | −4.27 | 28.4 | – |
per 1 mol of Potassium sulfate ion | 4.23 | −4.27 | 28.4 | – |
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 |
|---|---|---|---|---|
| K+ (g) | 514.26[1] | – | – | – |
| K+ (ao) | -252.38[1] | -283.27[1] | 102.5[1] | 21.8[1] |
| SO42− (ao) | -909.27[1] | -744.53[1] | 20.1[1] | -293[1] |
* (g):Gas, (ao):Un-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 |
|---|---|---|---|---|
| KSO4− (ao) | -1157.42[1] | -1032.07[1] | 151.0[1] | – |
* (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°, 514.26 kJ · mol−1
- ^ ΔfH°, -252.38 kJ · mol−1
- ^ ΔfG°, -283.27 kJ · mol−1
- ^ S°, 102.5 J · K−1 · mol−1
- ^ Cp°, 21.8 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
- ^ ΔfH°, -1157.42 kJ · mol−1
- ^ ΔfG°, -1032.07 kJ · mol−1
- ^ S°, 151.0 J · K−1 · mol−1