3NH4HSO4 + 2Al(OH)3 🔥→ Al2(SO4)3 + 3NH3↑ + 6H2O
Last updated:
The reaction of ammonium hydrogensulfate and aluminium hydroxide yields aluminium sulfate, ammonia, and water (Other reactions are here). This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of ammonium hydrogensulfate and aluminium hydroxide
General equation
- Reaction of volatile acid and non volatile base
- Salt of volatile baseBrønsted acid + Nonvolatile baseBrønsted base ⟶ Salt of non volatile baseConjugate acid + Volatile baseConjugate base + (H2O)
Oxidation state of each atom
- Reaction of ammonium hydrogensulfate and aluminium hydroxide
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| NH4HSO4 | Ammonium hydrogensulfate | 3 | Brønsted acid | Salt of volatile base |
| Al(OH)3 | Aluminium hydroxide | 2 | Brønsted base | Nonvolatile base |
Products
Thermodynamic changes
Changes in standard condition (1)
- Reaction of ammonium hydrogensulfate and aluminium hydroxide
| 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 | 355 | – | – | – |
per 1 mol of | 118 | – | – | – |
per 1 mol of | 178 | – | – | – |
per 1 mol of | 355 | – | – | – |
per 1 mol of | 118 | – | – | – |
per 1 mol of | 59.2 | – | – | – |
Changes in standard condition (2)
- Reaction of ammonium hydrogensulfate and aluminium hydroxide
| 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 | 339 | – | – | – |
per 1 mol of | 113 | – | – | – |
per 1 mol of | 170 | – | – | – |
per 1 mol of | 339 | – | – | – |
per 1 mol of | 113 | – | – | – |
per 1 mol of | 56.5 | – | – | – |
Changes in aqueous solution (1)
- Reaction of ammonium hydrogensulfate and aluminium hydroxide
| 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 | −1 | – | – | – |
per 1 mol of | −0.3 | – | – | – |
per 1 mol of | −0.5 | – | – | – |
per 1 mol of | −1 | – | – | – |
per 1 mol of | −0.3 | – | – | – |
per 1 mol of | −0.2 | – | – | – |
Changes in aqueous solution (2)
- Reaction of ammonium hydrogensulfate and aluminium hydroxide
| 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 | −103 | – | – | – |
per 1 mol of | −34.3 | – | – | – |
per 1 mol of | −51.5 | – | – | – |
per 1 mol of | −103 | – | – | – |
per 1 mol of | −34.3 | – | – | – |
per 1 mol of | −17.2 | – | – | – |
Changes in aqueous solution (3)
- Reaction of ammonium hydrogensulfate and aluminium hydroxide◆
ΔrG 441 kJ/mol K 0.55 × 10−77 pK 77.26
| 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 | −17 | 441 | −464 | – |
per 1 mol of | −5.7 | 147 | −155 | – |
per 1 mol of | −8.5 | 221 | −232 | – |
per 1 mol of | −17 | 441 | −464 | – |
per 1 mol of | −5.7 | 147 | −155 | – |
per 1 mol of | −2.8 | 73.5 | −77.3 | – |
Changes in aqueous solution (4)
- Reaction of ammonium hydrogensulfate and aluminium hydroxide◆
ΔrG 410 kJ/mol K 0.15 × 10−71 pK 71.83
| 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 | −119 | 410 | −707 | – |
per 1 mol of | −39.7 | 137 | −236 | – |
per 1 mol of | −59.5 | 205 | −354 | – |
per 1 mol of | −119 | 410 | −707 | – |
per 1 mol of | −39.7 | 137 | −236 | – |
per 1 mol of | −19.8 | 68.3 | −118 | – |
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 |
|---|---|---|---|---|
| NH4HSO4 (cr) | -1026.96[1] | – | – | – |
| NH4HSO4 (ai) | -1019.85[1] | -835.21[1] | 245.2[1] | -3.8[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, (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 |
|---|---|---|---|---|
| Al2(SO4)3 (cr) | -3440.84[1] | -3099.94[1] | 239.3[1] | 259.41[1] |
| Al2(SO4)3 (ai) | -3791[1] | -3205[1] | -583.2[1] | – |
| Al2(SO4)3 (aq) | -3774.8[1] | – | – | – |
| Al2(SO4)3 (cr) 6 hydrate | -5311.71[1] | -4622.08[1] | 469.0[1] | 492.9[1] |
| Al2(SO4)3 (cr) 18 hydrate | -8878.9[1] | – | – | – |
| NH3 (g) | -46.11[1] | -16.45[1] | 192.45[1] | 35.06[1] |
| NH3 (ao) | -80.29[1] | -26.50[1] | 111.3[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, (ai):Ionized aqueous solution, (aq):Aqueous solution, (g):Gas, (ao):Un-ionized aqueous solution, (l):Liquid
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°, -1026.96 kJ · mol−1
- ^ ΔfH°, -1019.85 kJ · mol−1
- ^ ΔfG°, -835.21 kJ · mol−1
- ^ S°, 245.2 J · K−1 · mol−1
- ^ Cp°, -3.8 J · K−1 · mol−1
- ^ ΔfH°, -1276. kJ · mol−1
- ^ ΔfH°, -3440.84 kJ · mol−1
- ^ ΔfG°, -3099.94 kJ · mol−1
- ^ S°, 239.3 J · K−1 · mol−1
- ^ Cp°, 259.41 J · K−1 · mol−1
- ^ ΔfH°, -3791. kJ · mol−1
- ^ ΔfG°, -3205. kJ · mol−1
- ^ S°, -583.2 J · K−1 · mol−1
- ^ ΔfH°, -3774.8 kJ · mol−1
- ^ ΔfH°, -5311.71 kJ · mol−1
- ^ ΔfG°, -4622.08 kJ · mol−1
- ^ S°, 469.0 J · K−1 · mol−1
- ^ Cp°, 492.9 J · K−1 · mol−1
- ^ ΔfH°, -8878.9 kJ · mol−1
- ^ ΔfH°, -46.11 kJ · mol−1
- ^ ΔfG°, -16.45 kJ · mol−1
- ^ S°, 192.45 J · K−1 · mol−1
- ^ Cp°, 35.06 J · K−1 · mol−1
- ^ ΔfH°, -80.29 kJ · mol−1
- ^ ΔfG°, -26.50 kJ · mol−1
- ^ S°, 111.3 J · K−1 · 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
- 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