2NaH2PO4 + 2e− → Na2HPO4 + H2PO4− + H−
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- Reduction of sodium dihydrogenphosphate
- 2NaH2PO4Sodium dihydrogenphosphate + 2e−ElectronNa2HPO4Sodium hydrogenphosphate + H2PO4−Dihydrogenphosphate ion + H−Hydride ion⟶
Reduction of sodium dihydrogenphosphate yields sodium hydrogenphosphate, dihydrogenphosphate ion, and hydride ion (Other reactions are here). This reaction is an oxidation-reduction reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reduction of sodium dihydrogenphosphate
- 2NaH2PO4Sodium dihydrogenphosphate + 2e−ElectronNa2HPO4Sodium hydrogenphosphate + H2PO4−Dihydrogenphosphate ion + H−Hydride ion⟶
General equation
- Reduction of reducible species
- ReactantOxidizing agent + e− ⟶ ProductReduction product
Oxidation state of each atom
- Reduction of sodium dihydrogenphosphate
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| NaH2PO4 | Sodium dihydrogenphosphate | 2 | Oxidizing | – |
| e− | Electron | 2 | – | Electron |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Na2HPO4 | Sodium hydrogenphosphate | 1 | – | – |
| H2PO4− | Dihydrogenphosphate ion | 1 | – | – |
| H− | Hydride ion | 1 | Reduced | – |
Thermodynamic changes
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 |
|---|---|---|---|---|
| NaH2PO4 (cr) | -1536.8[1] | -1386.1[1] | 127.49[1] | 116.86[1] |
| NaH2PO4 (ai) | -1536.41[1] | -1392.17[1] | 149.4[1] | – |
| NaH2PO4 (cr) 1 hydrate | -1833.0[1] | – | – | – |
| NaH2PO4 (cr) 2 hydrate | -2128.4[1] | – | – | – |
| e− | – | – | – | – |
* (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 |
|---|---|---|---|---|
| Na2HPO4 (cr) | -1748.1[1] | -1608.2[1] | 150.50[1] | 135.31[1] |
| Na2HPO4 (ai) | -1772.38[1] | -1612.98[1] | 84.5[1] | – |
| Na2HPO4 (cr) 2 hydrate | -2346.0[1] | -2088.5[1] | 221.3[1] | – |
| Na2HPO4 (cr) 7 hydrate | -3821.7[1] | -3279.8[1] | 434.59[1] | – |
| Na2HPO4 (cr) 12 hydrate | -5297.8[1] | -4467.8[1] | 633.83[1] | – |
| H2PO4− (ao) | -1296.29[1] | -1130.28[1] | 90.4[1] | – |
| H− (g) | 138.99[1] | – | – | – |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution, (g):Gas
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°, -1536.8 kJ · mol−1
- ^ ΔfG°, -1386.1 kJ · mol−1
- ^ S°, 127.49 J · K−1 · mol−1
- ^ Cp°, 116.86 J · K−1 · mol−1
- ^ ΔfH°, -1536.41 kJ · mol−1
- ^ ΔfG°, -1392.17 kJ · mol−1
- ^ S°, 149.4 J · K−1 · mol−1
- ^ ΔfH°, -1833.0 kJ · mol−1
- ^ ΔfH°, -2128.4 kJ · mol−1
- ^ ΔfH°, -1748.1 kJ · mol−1
- ^ ΔfG°, -1608.2 kJ · mol−1
- ^ S°, 150.50 J · K−1 · mol−1
- ^ Cp°, 135.31 J · K−1 · mol−1
- ^ ΔfH°, -1772.38 kJ · mol−1
- ^ ΔfG°, -1612.98 kJ · mol−1
- ^ S°, 84.5 J · K−1 · mol−1
- ^ ΔfH°, -2346.0 kJ · mol−1
- ^ ΔfG°, -2088.5 kJ · mol−1
- ^ S°, 221.3 J · K−1 · mol−1
- ^ ΔfH°, -3821.7 kJ · mol−1
- ^ ΔfG°, -3279.8 kJ · mol−1
- ^ S°, 434.59 J · K−1 · mol−1
- ^ ΔfH°, -5297.8 kJ · mol−1
- ^ ΔfG°, -4467.8 kJ · mol−1
- ^ S°, 633.83 J · K−1 · mol−1
- ^ ΔfH°, -1296.29 kJ · mol−1
- ^ ΔfG°, -1130.28 kJ · mol−1
- ^ S°, 90.4 J · K−1 · mol−1
- ^ ΔfH°, 138.99 kJ · mol−1