FeF3 + H3PO4 🔥→ FePO4 + 3HF↑
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The reaction of iron(III) fluoride and phosphoric acid yields iron(III) phosphate and hydrogen fluoride. This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of iron(III) fluoride and phosphoric acid
General equation
- Salt of volatile acidBrønsted base + Nonvolatile acidBrønsted acid ⟶ Salt of non volatile acidConjugate base + Volatile acidConjugate acid
Oxidation state of each atom
- Reaction of iron(III) fluoride and phosphoric acid
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| FeF3 | Iron(III) fluoride | 1 | Brønsted base | Salt of volatile acid |
| H3PO4 | Phosphoric acid | 1 | Brønsted acid | Nonvolatile acid |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| FePO4 | Iron(III) phosphate | 1 | Conjugate base | Salt of non volatile acid |
| HF | Hydrogen fluoride | 3 | Conjugate acid | Volatile acid |
Thermodynamic changes
Changes in aqueous solution (1)
- Reaction of iron(III) fluoride and phosphoric acid
| 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 | 193.8 | – | – | – |
per 1 mol of | 193.8 | – | – | – |
per 1 mol of | 193.8 | – | – | – |
per 1 mol of | 193.8 | – | – | – |
per 1 mol of | 64.60 | – | – | – |
Changes in aqueous solution (2)
- Reaction of iron(III) fluoride and phosphoric acid
| 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 | 46.9 | – | – | – |
per 1 mol of | 46.9 | – | – | – |
per 1 mol of | 46.9 | – | – | – |
per 1 mol of | 46.9 | – | – | – |
per 1 mol of | 15.6 | – | – | – |
Changes in aqueous solution (3)
- Reaction of iron(III) fluoride and phosphoric acid
| 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 | 46.9 | – | – | – |
per 1 mol of | 46.9 | – | – | – |
per 1 mol of | 46.9 | – | – | – |
per 1 mol of | 46.9 | – | – | – |
per 1 mol of | 15.6 | – | – | – |
Changes in aqueous solution (4)
- Reaction of iron(III) fluoride and phosphoric acid
| 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 | 182.9 | – | – | – |
per 1 mol of | 182.9 | – | – | – |
per 1 mol of | 182.9 | – | – | – |
per 1 mol of | 182.9 | – | – | – |
per 1 mol of | 60.97 | – | – | – |
Changes in aqueous solution (5)
- Reaction of iron(III) fluoride and phosphoric acid
| 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 | 36.0 | – | – | – |
per 1 mol of | 36.0 | – | – | – |
per 1 mol of | 36.0 | – | – | – |
per 1 mol of | 36.0 | – | – | – |
per 1 mol of | 12.0 | – | – | – |
Changes in aqueous solution (6)
- Reaction of iron(III) fluoride and phosphoric acid
| 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 | 36.0 | – | – | – |
per 1 mol of | 36.0 | – | – | – |
per 1 mol of | 36.0 | – | – | – |
per 1 mol of | 36.0 | – | – | – |
per 1 mol of | 12.0 | – | – | – |
Changes in aqueous solution (7)
- Reaction of iron(III) fluoride and phosphoric acid
| 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 | 193.8 | – | – | – |
per 1 mol of | 193.8 | – | – | – |
per 1 mol of | 193.8 | – | – | – |
per 1 mol of | 193.8 | – | – | – |
per 1 mol of | 64.60 | – | – | – |
Changes in aqueous solution (8)
- Reaction of iron(III) fluoride and phosphoric acid
| 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 | 46.9 | – | – | – |
per 1 mol of | 46.9 | – | – | – |
per 1 mol of | 46.9 | – | – | – |
per 1 mol of | 46.9 | – | – | – |
per 1 mol of | 15.6 | – | – | – |
Changes in aqueous solution (9)
- Reaction of iron(III) fluoride and phosphoric acid
| 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 | 46.9 | – | – | – |
per 1 mol of | 46.9 | – | – | – |
per 1 mol of | 46.9 | – | – | – |
per 1 mol of | 46.9 | – | – | – |
per 1 mol of | 15.6 | – | – | – |
Changes in aqueous solution (10)
- Reaction of iron(III) fluoride and phosphoric acid
| 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 | 223.9 | – | – | – |
per 1 mol of | 223.9 | – | – | – |
per 1 mol of | 223.9 | – | – | – |
per 1 mol of | 223.9 | – | – | – |
per 1 mol of | 74.63 | – | – | – |
Changes in aqueous solution (11)
- Reaction of iron(III) fluoride and phosphoric acid
| 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 | 77.0 | – | – | – |
per 1 mol of | 77.0 | – | – | – |
per 1 mol of | 77.0 | – | – | – |
per 1 mol of | 77.0 | – | – | – |
per 1 mol of | 25.7 | – | – | – |
Changes in aqueous solution (12)
- Reaction of iron(III) fluoride and phosphoric acid
| 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 | 77.0 | – | – | – |
per 1 mol of | 77.0 | – | – | – |
per 1 mol of | 77.0 | – | – | – |
per 1 mol of | 77.0 | – | – | – |
per 1 mol of | 25.7 | – | – | – |
Changes in aqueous solution (13)
- Reaction of iron(III) fluoride and phosphoric acid
| 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 | 213.0 | – | – | – |
per 1 mol of | 213.0 | – | – | – |
per 1 mol of | 213.0 | – | – | – |
per 1 mol of | 213.0 | – | – | – |
per 1 mol of | 71.00 | – | – | – |
Changes in aqueous solution (14)
- Reaction of iron(III) fluoride and phosphoric acid
| 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 | 66.1 | – | – | – |
per 1 mol of | 66.1 | – | – | – |
per 1 mol of | 66.1 | – | – | – |
per 1 mol of | 66.1 | – | – | – |
per 1 mol of | 22.0 | – | – | – |
Changes in aqueous solution (15)
- Reaction of iron(III) fluoride and phosphoric acid
| 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 | 66.1 | – | – | – |
per 1 mol of | 66.1 | – | – | – |
per 1 mol of | 66.1 | – | – | – |
per 1 mol of | 66.1 | – | – | – |
per 1 mol of | 22.0 | – | – | – |
Changes in aqueous solution (16)
- Reaction of iron(III) fluoride and phosphoric acid
| 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 | 223.9 | – | – | – |
per 1 mol of | 223.9 | – | – | – |
per 1 mol of | 223.9 | – | – | – |
per 1 mol of | 223.9 | – | – | – |
per 1 mol of | 74.63 | – | – | – |
Changes in aqueous solution (17)
- Reaction of iron(III) fluoride and phosphoric acid
| 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 | 77.0 | – | – | – |
per 1 mol of | 77.0 | – | – | – |
per 1 mol of | 77.0 | – | – | – |
per 1 mol of | 77.0 | – | – | – |
per 1 mol of | 25.7 | – | – | – |
Changes in aqueous solution (18)
- Reaction of iron(III) fluoride and phosphoric acid
| 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 | 77.0 | – | – | – |
per 1 mol of | 77.0 | – | – | – |
per 1 mol of | 77.0 | – | – | – |
per 1 mol of | 77.0 | – | – | – |
per 1 mol of | 25.7 | – | – | – |
Changes in aqueous solution (19)
- Reaction of iron(III) fluoride and phosphoric acid
| 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 | 9.2 | – | – | – |
per 1 mol of | 9.2 | – | – | – |
per 1 mol of | 9.2 | – | – | – |
per 1 mol of | 9.2 | – | – | – |
per 1 mol of | 3.1 | – | – | – |
Changes in aqueous solution (20)
- Reaction of iron(III) fluoride and phosphoric acid
| 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 | −1.7 | – | – | – |
per 1 mol of | −1.7 | – | – | – |
per 1 mol of | −1.7 | – | – | – |
per 1 mol of | −1.7 | – | – | – |
per 1 mol of | −0.57 | – | – | – |
Changes in aqueous solution (21)
- Reaction of iron(III) fluoride and phosphoric acid
| 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 | 9.2 | – | – | – |
per 1 mol of | 9.2 | – | – | – |
per 1 mol of | 9.2 | – | – | – |
per 1 mol of | 9.2 | – | – | – |
per 1 mol of | 3.1 | – | – | – |
Changes in aqueous solution (22)
- Reaction of iron(III) fluoride and phosphoric acid
| 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 | 39.3 | – | – | – |
per 1 mol of | 39.3 | – | – | – |
per 1 mol of | 39.3 | – | – | – |
per 1 mol of | 39.3 | – | – | – |
per 1 mol of | 13.1 | – | – | – |
Changes in aqueous solution (23)
- Reaction of iron(III) fluoride and phosphoric acid
| 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 | 28.4 | – | – | – |
per 1 mol of | 28.4 | – | – | – |
per 1 mol of | 28.4 | – | – | – |
per 1 mol of | 28.4 | – | – | – |
per 1 mol of | 9.47 | – | – | – |
Changes in aqueous solution (24)
- Reaction of iron(III) fluoride and phosphoric acid
| 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 | 39.3 | – | – | – |
per 1 mol of | 39.3 | – | – | – |
per 1 mol of | 39.3 | – | – | – |
per 1 mol of | 39.3 | – | – | – |
per 1 mol of | 13.1 | – | – | – |
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 |
|---|---|---|---|---|
| FeF3 (ai) | -1046.4[1] | -840.9[1] | -357.3[1] | – |
| FeF3 (aq) | -1016.3[1] | – | – | – |
| H3PO4 (cr) | -1279.0[1] | -1119.1[1] | 110.50[1] | 106.06[1] |
| H3PO4 (l) | -1266.9[1] | – | – | – |
| H3PO4 (ai) | -1277.4[1] | -1018.7[1] | -220.3[1] | – |
| H3PO4 (ao) | -1288.34[1] | -1142.54[1] | 158.2[1] | – |
| H3PO4 (cr) 0.5 hydrate | -1431.3[1] | -1242.1[1] | 129.16[1] | 126.02[1] |
| H3PO4 (cr) 1 hydrate | -1568.83[1] | – | – | – |
* (ai):Ionized aqueous solution, (aq):Aqueous solution, (cr):Crystalline solid, (l):Liquid, (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 |
|---|---|---|---|---|
| FePO4 (cr) | -1297.5[1] | – | – | – |
| FePO4 (cr) 2 hydrate strengite | -1888.2[1] | -1657.5[1] | 171.25[1] | 180.54[1] |
| HF (l) x denotes undetermined zero point entropy | -299.78[1] | – | 75.40+x[1] | – |
| HF (g) | -271.1[1] | -273.2[1] | 173.779[1] | 29.133[1] |
| HF (ai) | -332.63[1] | -278.79[1] | -13.8[1] | -106.7[1] |
| HF (ao) | -320.08[1] | -296.82[1] | 88.7[1] | – |
* (cr):Crystalline solid, (l):Liquid, (g):Gas, (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°, -1046.4 kJ · mol−1
- ^ ΔfG°, -840.9 kJ · mol−1
- ^ S°, -357.3 J · K−1 · mol−1
- ^ ΔfH°, -1016.3 kJ · mol−1
- ^ ΔfH°, -1279.0 kJ · mol−1
- ^ ΔfG°, -1119.1 kJ · mol−1
- ^ S°, 110.50 J · K−1 · mol−1
- ^ Cp°, 106.06 J · K−1 · mol−1
- ^ ΔfH°, -1266.9 kJ · mol−1
- ^ ΔfH°, -1277.4 kJ · mol−1
- ^ ΔfG°, -1018.7 kJ · mol−1
- ^ S°, -220.3 J · K−1 · mol−1
- ^ ΔfH°, -1288.34 kJ · mol−1
- ^ ΔfG°, -1142.54 kJ · mol−1
- ^ S°, 158.2 J · K−1 · mol−1
- ^ ΔfH°, -1431.3 kJ · mol−1
- ^ ΔfG°, -1242.1 kJ · mol−1
- ^ S°, 129.16 J · K−1 · mol−1
- ^ Cp°, 126.02 J · K−1 · mol−1
- ^ ΔfH°, -1568.83 kJ · mol−1
- ^ ΔfH°, -1297.5 kJ · mol−1
- ^ ΔfH°, -1888.2 kJ · mol−1
- ^ ΔfG°, -1657.5 kJ · mol−1
- ^ S°, 171.25 J · K−1 · mol−1
- ^ Cp°, 180.54 J · K−1 · mol−1
- ^ ΔfH°, -299.78 kJ · mol−1
- ^ S°, 75.40+x J · K−1 · mol−1
- ^ ΔfH°, -271.1 kJ · mol−1
- ^ ΔfG°, -273.2 kJ · mol−1
- ^ S°, 173.779 J · K−1 · mol−1
- ^ Cp°, 29.133 J · K−1 · mol−1
- ^ ΔfH°, -332.63 kJ · mol−1
- ^ ΔfG°, -278.79 kJ · mol−1
- ^ S°, -13.8 J · K−1 · mol−1
- ^ Cp°, -106.7 J · K−1 · mol−1
- ^ ΔfH°, -320.08 kJ · mol−1
- ^ ΔfG°, -296.82 kJ · mol−1
- ^ S°, 88.7 J · K−1 · mol−1