H+ + HSeO3− → H2SeO3
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- Reaction of hydrogen ion and hydrogenselenite ion
The reaction of hydrogen ion and hydrogenselenite ion yields selenous acid (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 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 hydrogenselenite ion
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| H+ | Hydrogen ion | 1 | Lewis acid | Cation Hydrogen ion |
| HSeO3− | Hydrogenselenite ion | 1 | Lewis base | Anion |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| H2SeO3 | Selenous acid | 1 | Lewis conjugate | – Acid |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of hydrogen ion and hydrogenselenite ion◆
ΔrG −14.68 kJ/mol K 3.73 × 102 pK −2.57
| 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 | 7.07 | −14.68 | 72.8 | – |
per 1 mol of Hydrogen ion | 7.07 | −14.68 | 72.8 | – |
per 1 mol of Hydrogenselenite ion | 7.07 | −14.68 | 72.8 | – |
per 1 mol of | 7.07 | −14.68 | 72.8 | – |
Changes in standard condition (2)
- Reaction of hydrogen ion and hydrogenselenite ion
| 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 | 7.28 | – | – | – |
per 1 mol of Hydrogen ion | 7.28 | – | – | – |
per 1 mol of Hydrogenselenite ion | 7.28 | – | – | – |
per 1 mol of | 7.28 | – | – | – |
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] |
| HSeO3− (ao) | -514.55[1] | -411.46[1] | 135.1[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 |
|---|---|---|---|---|
| H2SeO3 (cr) | -524.46[1] | – | – | – |
| H2SeO3 (ao) | -507.48[1] | -426.14[1] | 207.9[1] | – |
| H2SeO3 (aq) | -507.27[1] | – | – | – |
* (cr):Crystalline solid, (ao):Un-ionized aqueous solution, (aq):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°, 1536.202 kJ · mol−1
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 0 J · K−1 · mol−1
- ^ Cp°, 0 J · K−1 · mol−1
- ^ ΔfH°, -514.55 kJ · mol−1
- ^ ΔfG°, -411.46 kJ · mol−1
- ^ S°, 135.1 J · K−1 · mol−1
- ^ ΔfH°, -524.46 kJ · mol−1
- ^ ΔfH°, -507.48 kJ · mol−1
- ^ ΔfG°, -426.14 kJ · mol−1
- ^ S°, 207.9 J · K−1 · mol−1
- ^ ΔfH°, -507.27 kJ · mol−1