2NaOH + Al2O3 + 3H2O → 2Na[Al(OH)4]
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The reaction of sodium hydroxide, aluminium oxide, and water yields sodium tetrahydroxydoaluminate. This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of sodium hydroxide, aluminium oxide, and water
General equation
- Reaction of base and amphoteric oxide
- BaseLewis base + Amphoteric oxideLewis acid + H2O ⟶ Salt of weak acidLewis conjugate + (H2O)
Oxidation state of each atom
- Reaction of sodium hydroxide, aluminium oxide, and water
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| NaOH | Sodium hydroxide | 2 | Lewis base | Base |
| Al2O3 | Aluminium oxide | 1 | Lewis acid | Amphoteric oxide |
| H2O | Water | 3 | – | Water |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Na[Al(OH)4] | Sodium tetrahydroxydoaluminate | 2 | Lewis conjugate | Salt of weak acid |
Thermodynamic changes
Changes in standard condition
- Reaction of sodium hydroxide, aluminium oxide, and water◆
ΔrG −2.4 kJ/mol K 2.63 × 100 pK −0.42 - 2NaOHIonized aqueous solution + Al2O3Crystalline solidα, corundum + 3H2OLiquid2Na[Al(OH)4]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 | −11.8 | −2.4 | −33.1 | – |
per 1 mol of | −5.90 | −1.2 | −16.6 | – |
per 1 mol of | −11.8 | −2.4 | −33.1 | – |
per 1 mol of | −3.93 | −0.80 | −11.0 | – |
per 1 mol of | −5.90 | −1.2 | −16.6 | – |
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 |
|---|---|---|---|---|
| NaOH (cr) | -425.609[1] | -379.494[1] | 64.455[1] | 59.54[1] |
| NaOH (g) | -207.1[1] | -210.0[1] | 228.43[1] | 48.37[1] |
| NaOH (ai) | -470.114[1] | -419.150[1] | 48.1[1] | -102.1[1] |
| NaOH (cr) 1 hydrate | -734.543[1] | -629.338[1] | 99.50[1] | 90.17[1] |
| NaOH (l) 2 hydrate | -1019.076[1] | -873.091[1] | 195.979[1] | 239.41[1] |
| NaOH (l) 3.5 hydrate | -1459.798[1] | -1236.356[1] | 286.089[1] | 354.43[1] |
| NaOH (l) 4 hydrate | -1605.15[1] | -1356.64[1] | 318.70[1] | – |
| NaOH (l) 5 hydrate | -1894.31[1] | -1596.34[1] | 386.06[1] | – |
| NaOH (l) 7 hydrate | -2469.02[1] | -2073.80[1] | 526.31[1] | – |
| Al2O3 (cr) α, corundum | -1675.7[1] | -1582.3[1] | 50.92[1] | 79.04[1] |
| Al2O3 (cr) δ | -1666.5[1] | – | – | – |
| Al2O3 (cr) ρ | -1657[1] | – | – | – |
| Al2O3 (cr) κ | -1662.3[1] | – | – | – |
| Al2O3 (cr) γ | -1656.9[1] | – | – | – |
| Al2O3 (am) | -1632[1] | – | – | – |
| Al2O3 (cr) 1 hydrate | -1998.91[1] | -1841.78[1] | 70.67[1] | 106.19[1] |
| Al2O3 (cr) 3 hydrate | -2576.5[1] | – | – | – |
| H2O (cr) | – | – | – | – |
| H2O (l) | -285.830[1] | -237.129[1] | 69.91[1] | 75.291[1] |
| H2O (g) | -241.818[1] | -228.572[1] | 188.825[1] | 33.577[1] |
* (cr):Crystalline solid, (g):Gas, (ai):Ionized aqueous solution, (l):Liquid, (am):Amorphous solid
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 |
|---|---|---|---|---|
| Na[Al(OH)4] (ai) | -1742.6[1] | -1567.2[1] | 161.9[1] | – |
* (ai):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°, -425.609 kJ · mol−1
- ^ ΔfG°, -379.494 kJ · mol−1
- ^ S°, 64.455 J · K−1 · mol−1
- ^ Cp°, 59.54 J · K−1 · mol−1
- ^ ΔfH°, -207.1 kJ · mol−1
- ^ ΔfG°, -210.0 kJ · mol−1
- ^ S°, 228.43 J · K−1 · mol−1
- ^ Cp°, 48.37 J · K−1 · mol−1
- ^ ΔfH°, -470.114 kJ · mol−1
- ^ ΔfG°, -419.150 kJ · mol−1
- ^ S°, 48.1 J · K−1 · mol−1
- ^ Cp°, -102.1 J · K−1 · mol−1
- ^ ΔfH°, -734.543 kJ · mol−1
- ^ ΔfG°, -629.338 kJ · mol−1
- ^ S°, 99.50 J · K−1 · mol−1
- ^ Cp°, 90.17 J · K−1 · mol−1
- ^ ΔfH°, -1019.076 kJ · mol−1
- ^ ΔfG°, -873.091 kJ · mol−1
- ^ S°, 195.979 J · K−1 · mol−1
- ^ Cp°, 239.41 J · K−1 · mol−1
- ^ ΔfH°, -1459.798 kJ · mol−1
- ^ ΔfG°, -1236.356 kJ · mol−1
- ^ S°, 286.089 J · K−1 · mol−1
- ^ Cp°, 354.43 J · K−1 · mol−1
- ^ ΔfH°, -1605.15 kJ · mol−1
- ^ ΔfG°, -1356.64 kJ · mol−1
- ^ S°, 318.70 J · K−1 · mol−1
- ^ ΔfH°, -1894.31 kJ · mol−1
- ^ ΔfG°, -1596.34 kJ · mol−1
- ^ S°, 386.06 J · K−1 · mol−1
- ^ ΔfH°, -2469.02 kJ · mol−1
- ^ ΔfG°, -2073.80 kJ · mol−1
- ^ S°, 526.31 J · K−1 · mol−1
- ^ ΔfH°, -1675.7 kJ · mol−1
- ^ ΔfG°, -1582.3 kJ · mol−1
- ^ S°, 50.92 J · K−1 · mol−1
- ^ Cp°, 79.04 J · K−1 · mol−1
- ^ ΔfH°, -1666.5 kJ · mol−1
- ^ ΔfH°, -1657. kJ · mol−1
- ^ ΔfH°, -1662.3 kJ · mol−1
- ^ ΔfH°, -1656.9 kJ · mol−1
- ^ ΔfH°, -1632. kJ · mol−1
- ^ ΔfH°, -1998.91 kJ · mol−1
- ^ ΔfG°, -1841.78 kJ · mol−1
- ^ S°, 70.67 J · K−1 · mol−1
- ^ Cp°, 106.19 J · K−1 · mol−1
- ^ ΔfH°, -2576.5 kJ · mol−1
- ^ ΔfH°, -285.830 kJ · mol−1
- ^ ΔfG°, -237.129 kJ · mol−1
- ^ S°, 69.91 J · K−1 · mol−1
- ^ Cp°, 75.291 J · K−1 · mol−1
- ^ ΔfH°, -241.818 kJ · mol−1
- ^ ΔfG°, -228.572 kJ · mol−1
- ^ S°, 188.825 J · K−1 · mol−1
- ^ Cp°, 33.577 J · K−1 · mol−1
- ^ ΔfH°, -1742.6 kJ · mol−1
- ^ ΔfG°, -1567.2 kJ · mol−1
- ^ S°, 161.9 J · K−1 · mol−1