Fe2(SO4)3 + 3Sr(OH)2 → 3SrSO4↓ + 2Fe(OH)3↓
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The reaction of iron(III) sulfate and strontium hydroxide yields strontium sulfate and iron(III) hydroxide. 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 strontium 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)
- 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 iron(III) sulfate and strontium hydroxide
Reactants
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
Fe2(SO4)3 | Iron(III) sulfate | 1 | Brønsted acid Lewis acid | Salt of weak base Soluble in water |
Sr(OH)2 | Strontium hydroxide | 3 | Brønsted base Lewis base | Strong base Soluble in water |
Products
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
SrSO4 | Strontium sulfate | 3 | Conjugate acid Lewis conjugate | Salt of strong base Very slightly soluble in water |
Fe(OH)3 | Iron(III) hydroxide | 2 | Conjugate base Lewis conjugate | Weak base Insoluble in water |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of iron(III) sulfate and strontium 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 | −546.8 | – | – | – |
per 1 mol of | −546.8 | – | – | – |
per 1 mol of | −182.3 | – | – | – |
per 1 mol of | −182.3 | – | – | – |
per 1 mol of | −273.4 | – | – | – |
Changes in standard condition (2)
- Reaction of iron(III) sulfate and strontium 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 | −536.9 | – | – | – |
per 1 mol of | −536.9 | – | – | – |
per 1 mol of | −179.0 | – | – | – |
per 1 mol of | −179.0 | – | – | – |
per 1 mol of | −268.4 | – | – | – |
Changes in aqueous solution (1)
- Reaction of iron(III) sulfate and strontium 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 | – | – | – | – |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
Changes in aqueous solution (2)
- Reaction of iron(III) sulfate and strontium 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 | – | – | – | – |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
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] | – |
Sr(OH)2 (cr) | -959.0[1] | – | – | – |
Sr(OH)2 (g) | -565[1] | – | – | – |
Sr(OH)2 (cr) 1 hydrate | -1264.8[1] | – | – | – |
Sr(OH)2 (cr) 8 hydrate | -3352.2[1] | – | – | – |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (g):Gas
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 |
---|---|---|---|---|
SrSO4 (cr) | -1453.1[1] | -1340.9[1] | 117[1] | – |
SrSO4 (cr) precipitated | -1449.8[1] | – | – | – |
SrSO4 (ai) | -1455.07[1] | -1304.00[1] | -12.6[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°, -959.0 kJ · mol−1
- ^ ΔfH°, -565. kJ · mol−1
- ^ ΔfH°, -1264.8 kJ · mol−1
- ^ ΔfH°, -3352.2 kJ · mol−1
- ^ ΔfH°, -1453.1 kJ · mol−1
- ^ ΔfG°, -1340.9 kJ · mol−1
- ^ S°, 117. J · K−1 · mol−1
- ^ ΔfH°, -1449.8 kJ · mol−1
- ^ ΔfH°, -1455.07 kJ · mol−1
- ^ ΔfG°, -1304.00 kJ · mol−1
- ^ S°, -12.6 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