Fe2(SO4)3 + 6AgOH → 3Ag2SO4 + 2Fe(OH)3
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- Reaction of iron(III) sulfate and silver(I) hydroxide
- Fe2(SO4)3Iron(III) sulfate + 6AgOHSilver(I) hydroxide3Ag2SO4Silver(I) sulfate + 2Fe(OH)3Iron(III) hydroxide⟶
The reaction of iron(III) sulfate and silver(I) hydroxide yields silver(I) sulfate and iron(III) hydroxide (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 iron(III) sulfate and silver(I) hydroxide
- Fe2(SO4)3Iron(III) sulfate + 6AgOHSilver(I) hydroxide3Ag2SO4Silver(I) sulfate + 2Fe(OH)3Iron(III) 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 iron(III) sulfate and silver(I) hydroxide
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Fe2(SO4)3 | Iron(III) sulfate | 1 | Brønsted acid | Salt of weak base |
| AgOH | Silver(I) hydroxide | 6 | Brønsted base | Strong base |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Ag2SO4 | Silver(I) sulfate | 3 | Conjugate acid | Salt of strong base |
| Fe(OH)3 | Iron(III) hydroxide | 2 | Conjugate base | Weak base |
Thermodynamic changes
Changes in aqueous solution (1)
- Reaction of iron(III) sulfate and silver(I) hydroxide◆
ΔrG −365.9 kJ/mol K 1.27 × 1064 pK −64.10
| 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 | – | −365.9 | – | – |
per 1 mol of | – | −365.9 | – | – |
per 1 mol of Silver(I) hydroxide | – | −60.98 | – | – |
per 1 mol of | – | −122.0 | – | – |
per 1 mol of | – | −182.9 | – | – |
Changes in aqueous solution (2)
- Reaction of iron(III) sulfate and silver(I) hydroxide◆
ΔrG −294.7 kJ/mol K 4.26 × 1051 pK −51.63
| 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 | – | −294.7 | – | – |
per 1 mol of | – | −294.7 | – | – |
per 1 mol of Silver(I) hydroxide | – | −49.12 | – | – |
per 1 mol of | – | −98.23 | – | – |
per 1 mol of | – | −147.3 | – | – |
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 |
|---|---|---|---|---|
| Fe2(SO4)3 (cr) | -2581.5[1] | – | – | – |
| Fe2(SO4)3 (ai) | -2825.0[1] | -2242.8[1] | -571.5[1] | – |
| AgOH (ai) | -124.415[1] | -80.137[1] | 61.92[1] | -126.8[1] |
| AgOH (ao) | – | -92.0[1] | – | – |
* (cr):Crystalline solid, (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 |
|---|---|---|---|---|
| Ag2SO4 (cr) | -715.88[1] | -618.41[1] | 200.4[1] | 131.38[1] |
| Ag2SO4 (ai) | -698.10[1] | -590.30[1] | 165.7[1] | -251[1] |
| Fe(OH)3 (cr) precipitated | -823.0[1] | -696.5[1] | 106.7[1] | – |
| Fe(OH)3 (ao) | – | -659.3[1] | – | – |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (ao):Un-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°, -2581.5 kJ · mol−1
- ^ ΔfH°, -2825.0 kJ · mol−1
- ^ ΔfG°, -2242.8 kJ · mol−1
- ^ S°, -571.5 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°, -715.88 kJ · mol−1
- ^ ΔfG°, -618.41 kJ · mol−1
- ^ S°, 200.4 J · K−1 · mol−1
- ^ Cp°, 131.38 J · K−1 · mol−1
- ^ ΔfH°, -698.10 kJ · mol−1
- ^ ΔfG°, -590.30 kJ · mol−1
- ^ S°, 165.7 J · K−1 · mol−1
- ^ Cp°, -251. J · K−1 · mol−1
- ^ ΔfH°, -823.0 kJ · mol−1
- ^ ΔfG°, -696.5 kJ · mol−1
- ^ S°, 106.7 J · K−1 · mol−1
- ^ ΔfG°, -659.3 kJ · mol−1