2AgF + H2SO4 → Ag2SO4↓ + 2HF↑
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- Reaction of silver(I) fluoride and sulfuric acid
The reaction of silver(I) fluoride and sulfuric acid yields silver(I) sulfate and hydrogen fluoride. This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of silver(I) fluoride and sulfuric acid
General equation
- Salt of volatile acidBrønsted base + Nonvolatile acidBrønsted acid ⟶ Salt of non volatile acidConjugate base + Volatile acidConjugate acid
- 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 silver(I) fluoride and sulfuric acid
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| AgF | Silver(I) fluoride | 2 | Brønsted base Lewis acid | Salt of volatile acid Very soluble in water |
| H2SO4 | Sulfuric acid | 1 | Brønsted acid Lewis base | Nonvolatile acid Miscible with water |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Ag2SO4 | Silver(I) sulfate | 1 | Conjugate base Lewis conjugate | Salt of non volatile acid Slightly soluble in water |
| HF | Hydrogen fluoride | 2 | Conjugate acid Non-redox product | Volatile acid – |
Thermodynamic changes
Changes in standard condition
- Reaction of silver(I) fluoride and sulfuric 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 | −34.9 | – | – | – |
per 1 mol of | −17.4 | – | – | – |
per 1 mol of | −34.9 | – | – | – |
per 1 mol of | −34.9 | – | – | – |
per 1 mol of | −17.4 | – | – | – |
Changes in aqueous solution (1)
- Reaction of silver(I) fluoride and sulfuric acid◆
ΔrG 11.2 kJ/mol K 0.11 × 10−1 pK 1.96
| 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 | 123.1 | 11.2 | 375.2 | 270 |
per 1 mol of | 61.55 | 5.60 | 187.6 | 135 |
per 1 mol of | 123.1 | 11.2 | 375.2 | 270 |
per 1 mol of | 123.1 | 11.2 | 375.2 | 270 |
per 1 mol of | 61.55 | 5.60 | 187.6 | 135 |
Changes in aqueous solution (2)
- Reaction of silver(I) fluoride and sulfuric acid◆
ΔrG −36.03 kJ/mol K 2.05 × 106 pK −6.31
| 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 | 25.15 | −36.03 | 205.0 | – |
per 1 mol of | 12.57 | −18.02 | 102.5 | – |
per 1 mol of | 25.15 | −36.03 | 205.0 | – |
per 1 mol of | 25.15 | −36.03 | 205.0 | – |
per 1 mol of | 12.57 | −18.02 | 102.5 | – |
Changes in aqueous solution (3)
- Reaction of silver(I) fluoride and sulfuric acid◆
ΔrG −36.03 kJ/mol K 2.05 × 106 pK −6.31
| 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 | 25.15 | −36.03 | 205.0 | – |
per 1 mol of | 12.57 | −18.02 | 102.5 | – |
per 1 mol of | 25.15 | −36.03 | 205.0 | – |
per 1 mol of | 25.15 | −36.03 | 205.0 | – |
per 1 mol of | 12.57 | −18.02 | 102.5 | – |
Changes in aqueous solution (4)
- Reaction of silver(I) fluoride and sulfuric acid◆
ΔrG 15.2 kJ/mol K 0.22 × 10−2 pK 2.66
| 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 | 146.8 | 15.2 | 441.4 | – |
per 1 mol of | 73.40 | 7.60 | 220.7 | – |
per 1 mol of | 146.8 | 15.2 | 441.4 | – |
per 1 mol of | 146.8 | 15.2 | 441.4 | – |
per 1 mol of | 73.40 | 7.60 | 220.7 | – |
Changes in aqueous solution (5)
- Reaction of silver(I) fluoride and sulfuric acid◆
ΔrG −32.0 kJ/mol K 4.04 × 105 pK −5.61
| 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 | 48.8 | −32.0 | 271.2 | – |
per 1 mol of | 24.4 | −16.0 | 135.6 | – |
per 1 mol of | 48.8 | −32.0 | 271.2 | – |
per 1 mol of | 48.8 | −32.0 | 271.2 | – |
per 1 mol of | 24.4 | −16.0 | 135.6 | – |
Changes in aqueous solution (6)
- Reaction of silver(I) fluoride and sulfuric acid◆
ΔrG −32.0 kJ/mol K 4.04 × 105 pK −5.61
| 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 | 48.8 | −32.0 | 271.2 | – |
per 1 mol of | 24.4 | −16.0 | 135.6 | – |
per 1 mol of | 48.8 | −32.0 | 271.2 | – |
per 1 mol of | 48.8 | −32.0 | 271.2 | – |
per 1 mol of | 24.4 | −16.0 | 135.6 | – |
Changes in aqueous solution (7)
- Reaction of silver(I) fluoride and sulfuric acid◆
ΔrG 0.03 kJ/mol K 0.99 × 100 pK 0.01
| 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 | 0.05 | 0.03 | 0.0 | −2 |
per 1 mol of | 0.0250 | 0.0150 | 0.0 | −1 |
per 1 mol of | 0.0500 | 0.0300 | 0.0 | −2 |
per 1 mol of | 0.0500 | 0.0300 | 0.0 | −2 |
per 1 mol of | 0.0250 | 0.0150 | 0.0 | −1 |
Changes in aqueous solution (8)
- Reaction of silver(I) fluoride and sulfuric acid◆
ΔrG 4.0 kJ/mol K 0.20 × 100 pK 0.70
| 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 | 23.7 | 4.0 | 66.2 | – |
per 1 mol of | 11.8 | 2.0 | 33.1 | – |
per 1 mol of | 23.7 | 4.0 | 66.2 | – |
per 1 mol of | 23.7 | 4.0 | 66.2 | – |
per 1 mol of | 11.8 | 2.0 | 33.1 | – |
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 |
|---|---|---|---|---|
| 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] |
| H2SO4 (cr) | – | – | – | – |
| H2SO4 (l) | -813.989[1] | -690.003[1] | 156.904[1] | 138.91[1] |
| H2SO4 (ai) | -909.27[1] | -744.53[1] | 20.1[1] | -293[1] |
| H2SO4 (l) 1 hydrate | -1127.621[1] | -950.383[1] | 211.54[1] | 214.85[1] |
| H2SO4 (l) 2 hydrate | -1427.100[1] | -1199.650[1] | 276.40[1] | 260.83[1] |
| H2SO4 (l) 3 hydrate | -1720.402[1] | -1443.980[1] | 345.39[1] | 318.95[1] |
| H2SO4 (l) 4 hydrate | -2011.199[1] | -1685.863[1] | 414.59[1] | 382.21[1] |
| H2SO4 (l) 6.5 hydrate | -2733.256[1] | -2285.734[1] | 587.89[1] | 570.28[1] |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution, (l):Liquid
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] |
| 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, (ai):Ionized aqueous solution, (l):Liquid, (g):Gas, (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°, -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°, -813.989 kJ · mol−1
- ^ ΔfG°, -690.003 kJ · mol−1
- ^ S°, 156.904 J · K−1 · mol−1
- ^ Cp°, 138.91 J · K−1 · mol−1
- ^ ΔfH°, -909.27 kJ · mol−1
- ^ ΔfG°, -744.53 kJ · mol−1
- ^ S°, 20.1 J · K−1 · mol−1
- ^ Cp°, -293. J · K−1 · mol−1
- ^ ΔfH°, -1127.621 kJ · mol−1
- ^ ΔfG°, -950.383 kJ · mol−1
- ^ S°, 211.54 J · K−1 · mol−1
- ^ Cp°, 214.85 J · K−1 · mol−1
- ^ ΔfH°, -1427.100 kJ · mol−1
- ^ ΔfG°, -1199.650 kJ · mol−1
- ^ S°, 276.40 J · K−1 · mol−1
- ^ Cp°, 260.83 J · K−1 · mol−1
- ^ ΔfH°, -1720.402 kJ · mol−1
- ^ ΔfG°, -1443.980 kJ · mol−1
- ^ S°, 345.39 J · K−1 · mol−1
- ^ Cp°, 318.95 J · K−1 · mol−1
- ^ ΔfH°, -2011.199 kJ · mol−1
- ^ ΔfG°, -1685.863 kJ · mol−1
- ^ S°, 414.59 J · K−1 · mol−1
- ^ Cp°, 382.21 J · K−1 · mol−1
- ^ ΔfH°, -2733.256 kJ · mol−1
- ^ ΔfG°, -2285.734 kJ · mol−1
- ^ S°, 587.89 J · K−1 · mol−1
- ^ Cp°, 570.28 J · K−1 · 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°, -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