SnCl2 + 2Na[Al(OH)4] 💧→ Sn(OH)2↓ + 2Al(OH)3↓ + 2NaCl
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The reaction of tin(II) chloride and sodium tetrahydroxydoaluminate yields tin(II) hydroxide, aluminium hydroxide, and sodium chloride. This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of tin(II) chloride and sodium tetrahydroxydoaluminate
General equation
- Precipitation reaction
- Miscible with water/Very soluble in water/Soluble in waterLewis acid + Miscible with water/Very soluble in water/Soluble in waterLewis base💧⟶ Insoluble in water/Very slightly soluble in water/Slightly soluble in waterLewis conjugate + Product(Non-redox product)
Oxidation state of each atom
- Reaction of tin(II) chloride and sodium tetrahydroxydoaluminate
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| SnCl2 | Tin(II) chloride | 1 | Lewis acid | Very soluble in water |
| Na[Al(OH)4] | Sodium tetrahydroxydoaluminate | 2 | Lewis base | Very soluble in water |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Sn(OH)2 | Tin(II) hydroxide | 1 | Lewis conjugate | Insoluble in water |
| Al(OH)3 | Aluminium hydroxide | 2 | Lewis conjugate | Insoluble in water |
| NaCl | Sodium chloride | 2 | Non-redox product | – |
Thermodynamic changes
Changes in standard condition
- Reaction of tin(II) chloride and sodium tetrahydroxydoaluminate
- SnCl2Crystalline solid + 2Na[Al(OH)4]Ionized aqueous solutionSn(OH)2↓Crystalline solidprecipitated + 2Al(OH)3↓Crystalline solid + 2NaClIonized 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 | −133 | – | – | – |
per 1 mol of | −133 | – | – | – |
per 1 mol of | −66.5 | – | – | – |
per 1 mol of | −133 | – | – | – |
per 1 mol of | −66.5 | – | – | – |
per 1 mol of | −66.5 | – | – | – |
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 |
|---|---|---|---|---|
| SnCl2 (cr) | -325.1[1] | – | – | – |
| SnCl2 (cr) 2 hydrate | -921.3[1] | – | – | – |
| Na[Al(OH)4] (ai) | -1742.6[1] | -1567.2[1] | 161.9[1] | – |
* (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 |
|---|---|---|---|---|
| Sn(OH)2 (cr) precipitated | -561.1[1] | -491.6[1] | 155[1] | – |
| Al(OH)3 (cr) | -1284[2] | -1306[2] | 71[2] | 93.1[2] |
| Al(OH)3 (am) | -1276[1] | – | – | – |
| NaCl (cr) | -411.153[1] | -384.138[1] | 72.13[1] | 50.50[1] |
| NaCl (g) | -176.65[1] | -196.66[1] | 229.81[1] | 35.77[1] |
| NaCl (ai) | -407.27[1] | -393.133[1] | 115.5[1] | -90.0[1] |
* (cr):Crystalline solid, (am):Amorphous solid, (g):Gas, (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°, -325.1 kJ · mol−1
- ^ ΔfH°, -921.3 kJ · mol−1
- ^ ΔfH°, -1742.6 kJ · mol−1
- ^ ΔfG°, -1567.2 kJ · mol−1
- ^ S°, 161.9 J · K−1 · mol−1
- ^ ΔfH°, -561.1 kJ · mol−1
- ^ ΔfG°, -491.6 kJ · mol−1
- ^ S°, 155. J · K−1 · mol−1
- ^ ΔfH°, -1276. kJ · mol−1
- ^ ΔfH°, -411.153 kJ · mol−1
- ^ ΔfG°, -384.138 kJ · mol−1
- ^ S°, 72.13 J · K−1 · mol−1
- ^ Cp°, 50.50 J · K−1 · mol−1
- ^ ΔfH°, -176.65 kJ · mol−1
- ^ ΔfG°, -196.66 kJ · mol−1
- ^ S°, 229.81 J · K−1 · mol−1
- ^ Cp°, 35.77 J · K−1 · mol−1
- ^ ΔfH°, -407.27 kJ · mol−1
- ^ ΔfG°, -393.133 kJ · mol−1
- ^ S°, 115.5 J · K−1 · mol−1
- ^ Cp°, -90.0 J · K−1 · mol−1
- 2James G. Speight (2017)Lange's Handbook of Chemistry, 17th editionMcGraw Hill Education
- ^ ΔfH°, -1284 kJ · mol−1 - p.254
- ^ ΔfG°, -1306 kJ · mol−1 - p.254
- ^ S°, 71 J · K−1 · mol−1 - p.254
- ^ Cp°, 93.1 J · K−1 · mol−1 - p.254