AlF3 + 3AgOH → 3AgF + Al(OH)3
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- Reaction of aluminium fluoride and silver(I) hydroxide
- AlF3Aluminium fluoride + 3AgOHSilver(I) hydroxide3AgFSilver(I) fluoride + Al(OH)3Aluminium hydroxide⟶
The reaction of aluminium fluoride and silver(I) hydroxide yields silver(I) fluoride and aluminium hydroxide. This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of aluminium fluoride and silver(I) hydroxide
- AlF3Aluminium fluoride + 3AgOHSilver(I) hydroxide3AgFSilver(I) fluoride + Al(OH)3Aluminium hydroxide⟶
General equation
- Reaction of salt of weak base and strong base
- Salt of weak baseBrønsted acid + Strong baseBrønsted base ⟶ Salt of strong baseConjugate acid + Weak baseConjugate base + (H2O)
Oxidation state of each atom
- Reaction of aluminium fluoride and silver(I) hydroxide
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| AlF3 | Aluminium fluoride | 1 | Brønsted acid | Salt of weak base |
| AgOH | Silver(I) hydroxide | 3 | Brønsted base | Strong base |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| AgF | Silver(I) fluoride | 3 | Conjugate acid | Salt of strong base |
| Al(OH)3 | Aluminium hydroxide | 1 | Conjugate base | Weak base |
Thermodynamic changes
Changes in aqueous solution (1)
- Reaction of aluminium fluoride and silver(I) hydroxide◆
ΔrG −246 kJ/mol K 1.25 × 1043 pK −43.10
| 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 | −88 | −246 | −4 | 143.7 |
per 1 mol of | −88 | −246 | −4 | 143.7 |
per 1 mol of Silver(I) hydroxide | −29 | −82.0 | −1 | 47.90 |
per 1 mol of | −29 | −82.0 | −1 | 47.90 |
per 1 mol of | −88 | −246 | −4 | 143.7 |
Changes in aqueous solution (2)
- Reaction of aluminium fluoride and silver(I) hydroxide◆
ΔrG −252 kJ/mol K 1.41 × 1044 pK −44.15
| 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 | −123 | −252 | −104 | – |
per 1 mol of | −123 | −252 | −104 | – |
per 1 mol of Silver(I) hydroxide | −41.0 | −84.0 | −34.7 | – |
per 1 mol of | −41.0 | −84.0 | −34.7 | – |
per 1 mol of | −123 | −252 | −104 | – |
Changes in aqueous solution (3)
- Reaction of aluminium fluoride and silver(I) hydroxide◆
ΔrG −210 kJ/mol K 6.17 × 1036 pK −36.79
| 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 | – | −210 | – | – |
per 1 mol of | – | −210 | – | – |
per 1 mol of Silver(I) hydroxide | – | −70.0 | – | – |
per 1 mol of | – | −70.0 | – | – |
per 1 mol of | – | −210 | – | – |
Changes in aqueous solution (4)
- Reaction of aluminium fluoride and silver(I) hydroxide◆
ΔrG −216 kJ/mol K 6.94 × 1037 pK −37.84
| 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 | – | −216 | – | – |
per 1 mol of | – | −216 | – | – |
per 1 mol of Silver(I) hydroxide | – | −72.0 | – | – |
per 1 mol of | – | −72.0 | – | – |
per 1 mol of | – | −216 | – | – |
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 |
|---|---|---|---|---|
| AlF3 (cr) | -1504.1[1] | -1425.0[1] | 66.44[1] | 75.10[1] |
| AlF3 (g) | -1204.6[1] | -1188.2[1] | 277.1[1] | 62.63[1] |
| AlF3 (ai) | -1531[1] | -1322[1] | -363.2[1] | – |
| AlF3 (ao) | -1519[1] | -1414[1] | -25[1] | – |
| AgOH (ai) | -124.415[1] | -80.137[1] | 61.92[1] | -126.8[1] |
| AgOH (ao) | – | -92.0[1] | – | – |
* (cr):Crystalline solid, (g):Gas, (ai):Ionized aqueous solution, (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 |
|---|---|---|---|---|
| AgF (cr) | -204.6[1] | – | – | – |
| AgF (ai) | -227.07[1] | -201.69[1] | 59.0[1] | -84.9[1] |
| AgF (ao) | -238.9[1] | -203.7[1] | 25.9[1] | – |
| AgF (cr) 2 hydrate | -800.8[1] | -671.0[1] | 174.9[1] | 130[1] |
| AgF (cr) 4 hydrate | -1388.3[1] | -1147.0[1] | 268[1] | 209[1] |
| Al(OH)3 (cr) | -1284[2] | -1306[2] | 71[2] | 93.1[2] |
| Al(OH)3 (am) | -1276[1] | – | – | – |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution, (am):Amorphous solid
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°, -1504.1 kJ · mol−1
- ^ ΔfG°, -1425.0 kJ · mol−1
- ^ S°, 66.44 J · K−1 · mol−1
- ^ Cp°, 75.10 J · K−1 · mol−1
- ^ ΔfH°, -1204.6 kJ · mol−1
- ^ ΔfG°, -1188.2 kJ · mol−1
- ^ S°, 277.1 J · K−1 · mol−1
- ^ Cp°, 62.63 J · K−1 · mol−1
- ^ ΔfH°, -1531. kJ · mol−1
- ^ ΔfG°, -1322. kJ · mol−1
- ^ S°, -363.2 J · K−1 · mol−1
- ^ ΔfH°, -1519. kJ · mol−1
- ^ ΔfG°, -1414. kJ · mol−1
- ^ S°, -25. J · K−1 · mol−1
- ^ ΔfH°, -124.415 kJ · mol−1
- ^ ΔfG°, -80.137 kJ · mol−1
- ^ S°, 61.92 J · K−1 · mol−1
- ^ Cp°, -126.8 J · K−1 · mol−1
- ^ ΔfG°, -92.0 kJ · mol−1
- ^ ΔfH°, -204.6 kJ · mol−1
- ^ ΔfH°, -227.07 kJ · mol−1
- ^ ΔfG°, -201.69 kJ · mol−1
- ^ S°, 59.0 J · K−1 · mol−1
- ^ Cp°, -84.9 J · K−1 · mol−1
- ^ ΔfH°, -238.9 kJ · mol−1
- ^ ΔfG°, -203.7 kJ · mol−1
- ^ S°, 25.9 J · K−1 · mol−1
- ^ ΔfH°, -800.8 kJ · mol−1
- ^ ΔfG°, -671.0 kJ · mol−1
- ^ S°, 174.9 J · K−1 · mol−1
- ^ Cp°, 130. J · K−1 · mol−1
- ^ ΔfH°, -1388.3 kJ · mol−1
- ^ ΔfG°, -1147.0 kJ · mol−1
- ^ S°, 268. J · K−1 · mol−1
- ^ Cp°, 209. J · K−1 · mol−1
- ^ ΔfH°, -1276. kJ · 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