H2SeO4 + SeO42− → 2HSeO4−
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- Reaction of selenic acid and selenate ion
The reaction of selenic acid and selenate ion yields hydrogenselenate ion. This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of selenic acid and selenate ion
General equation
- Reaction of neutral species and anion
- CompoundLewis acid + AnionLewis base ⟶ AnionLewis conjugate
Oxidation state of each atom
- Reaction of selenic acid and selenate ion
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| H2SeO4 | Selenic acid | 1 | Lewis acid | Compound |
| SeO42− | Selenate ion | 1 | Lewis base | Anion |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| HSeO4− | Hydrogenselenate ion | 2 | Lewis conjugate | Anion |
Thermodynamic changes
Changes in standard condition
- Reaction of selenic acid and selenate 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 | −34.0 | – | – | – |
per 1 mol of | −34.0 | – | – | – |
per 1 mol of Selenate ion | −34.0 | – | – | – |
per 1 mol of Hydrogenselenate ion | −17.0 | – | – | – |
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 |
|---|---|---|---|---|
| H2SeO4 (cr) | -530.1[1] | – | – | – |
| H2SeO4 (cr) 1 hydrate | -840.6[1] | – | – | – |
| H2SeO4 (l) 1 hydrate | -820.5[1] | – | – | – |
| SeO42− (ao) | -599.1[1] | -441.3[1] | 54.0[1] | – |
* (cr):Crystalline solid, (l):Liquid, (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 |
|---|---|---|---|---|
| HSeO4− (ao) | -581.6[1] | -452.2[1] | 149.4[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)