H+ + SeO32− → HSeO3−
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- Reaction of hydrogen ion and selenite ion
- H+Hydrogen ion + SeO32−Selenite ionHSeO3−Hydrogenselenite ion⟶
The reaction of hydrogen ion and selenite ion yields hydrogenselenite 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 hydrogen ion and selenite ion
- H+Hydrogen ion + SeO32−Selenite ionHSeO3−Hydrogenselenite ion⟶
General equation
- Reaction of cation and anion
- CationLewis acid + AnionLewis base ⟶ ProductLewis conjugate + (H2O)
- Reaction of hydrogen ion and anion
- H+Lewis acid + AnionLewis base ⟶ Acid/Acid salt ionLewis conjugate + (H2O)
Oxidation state of each atom
- Reaction of hydrogen ion and selenite ion
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| H+ | Hydrogen ion | 1 | Lewis acid | Cation Hydrogen ion |
| SeO32− | Selenite ion | 1 | Lewis base | Anion |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| HSeO3− | Hydrogenselenite ion | 1 | Lewis conjugate | – Acid salt ion |
Thermodynamic changes
Changes in standard condition
- Reaction of hydrogen ion and selenite ion◆
ΔrG −41.7 kJ/mol K 2.02 × 107 pK −7.31 - H+Un-ionized aqueous solution + SeO32−Un-ionized aqueous solutionHSeO3−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 | −41.7 | 122 | – |
per 1 mol of Hydrogen ion | −5.3 | −41.7 | 122 | – |
per 1 mol of Selenite ion | −5.3 | −41.7 | 122 | – |
per 1 mol of Hydrogenselenite ion | −5.3 | −41.7 | 122 | – |
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 |
|---|---|---|---|---|
| H+ (g) | 1536.202[1] | – | – | – |
| H+ (ao) | 0[1] | 0[1] | 0[1] | 0[1] |
| SeO32− (ao) | -509.2[1] | -369.8[1] | 13[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 |
|---|---|---|---|---|
| HSeO3− (ao) | -514.55[1] | -411.46[1] | 135.1[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)