ZnCl2 + 2NH4F 💧→ ZnF2↓ + 2NH4Cl
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- Reaction of zinc chloride and ammonium fluoride
The reaction of zinc chloride and ammonium fluoride yields zinc fluoride and ammonium chloride. This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of zinc chloride and ammonium fluoride
General equation
- 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 zinc chloride and ammonium fluoride
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| ZnCl2 | Zinc chloride | 1 | Lewis acid | Very soluble in water |
| NH4F | Ammonium fluoride | 2 | Lewis base | Very soluble in water |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| ZnF2 | Zinc fluoride | 1 | Lewis conjugate | Slightly soluble in water |
| NH4Cl | Ammonium chloride | 2 | Non-redox product | – |
Thermodynamic changes
Changes in standard condition
- Reaction of zinc chloride and ammonium fluoride◆
ΔrG −52.3 kJ/mol K 1.45 × 109 pK −9.16
| 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 | −50.3 | −52.3 | 7.5 | 32.0 |
per 1 mol of | −50.3 | −52.3 | 7.5 | 32.0 |
per 1 mol of | −25.1 | −26.1 | 3.8 | 16.0 |
per 1 mol of | −50.3 | −52.3 | 7.5 | 32.0 |
per 1 mol of | −25.1 | −26.1 | 3.8 | 16.0 |
Changes in aqueous solution (1)
- Reaction of zinc chloride and ammonium fluoride◆
ΔrG −8.7 kJ/mol K 3.34 × 101 pK −1.52
| 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 | 54.8 | −8.7 | 213.5 | 232 |
per 1 mol of | 54.8 | −8.7 | 213.5 | 232 |
per 1 mol of | 27.4 | −4.3 | 106.8 | 116 |
per 1 mol of | 54.8 | −8.7 | 213.5 | 232 |
per 1 mol of | 27.4 | −4.3 | 106.8 | 116 |
Changes in aqueous solution (2)
- Reaction of zinc chloride and ammonium fluoride◆
ΔrG −14.5 kJ/mol K 3.47 × 102 pK −2.54
| 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 | – | −14.5 | – | – |
per 1 mol of | – | −14.5 | – | – |
per 1 mol of | – | −7.25 | – | – |
per 1 mol of | – | −14.5 | – | – |
per 1 mol of | – | −7.25 | – | – |
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 |
|---|---|---|---|---|
| ZnCl2 (cr) | -415.05[1] | -369.398[1] | 111.46[1] | 71.34[1] |
| ZnCl2 (g) | -266.1[1] | – | – | – |
| ZnCl2 (ai) | -488.19[1] | -409.50[1] | 0.8[1] | -226[1] |
| ZnCl2 (ao) | – | -403.7[1] | – | – |
| NH4F (cr) | -463.96[1] | -348.68[1] | 71.96[1] | 65.27[1] |
| NH4F (ai) | -465.14[1] | -358.09[1] | 99.6[1] | -26.8[1] |
* (cr):Crystalline solid, (g):Gas, (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 |
|---|---|---|---|---|
| ZnF2 (cr) | -764.4[1] | -713.3[1] | 73.68[1] | 65.65[1] |
| ZnF2 (ai) | -819.14[1] | -704.64[1] | -139.7[1] | -167[1] |
| NH4Cl (cr) | -314.43[1] | -202.87[1] | 94.6[1] | 84.1[1] |
| NH4Cl (ai) | -299.66[1] | -210.52[1] | 169.9[1] | -56.5[1] |
* (cr):Crystalline solid, (ai):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°, -415.05 kJ · mol−1
- ^ ΔfG°, -369.398 kJ · mol−1
- ^ S°, 111.46 J · K−1 · mol−1
- ^ Cp°, 71.34 J · K−1 · mol−1
- ^ ΔfH°, -266.1 kJ · mol−1
- ^ ΔfH°, -488.19 kJ · mol−1
- ^ ΔfG°, -409.50 kJ · mol−1
- ^ S°, 0.8 J · K−1 · mol−1
- ^ Cp°, -226. J · K−1 · mol−1
- ^ ΔfG°, -403.7 kJ · mol−1
- ^ ΔfH°, -463.96 kJ · mol−1
- ^ ΔfG°, -348.68 kJ · mol−1
- ^ S°, 71.96 J · K−1 · mol−1
- ^ Cp°, 65.27 J · K−1 · mol−1
- ^ ΔfH°, -465.14 kJ · mol−1
- ^ ΔfG°, -358.09 kJ · mol−1
- ^ S°, 99.6 J · K−1 · mol−1
- ^ Cp°, -26.8 J · K−1 · mol−1
- ^ ΔfH°, -764.4 kJ · mol−1
- ^ ΔfG°, -713.3 kJ · mol−1
- ^ S°, 73.68 J · K−1 · mol−1
- ^ Cp°, 65.65 J · K−1 · mol−1
- ^ ΔfH°, -819.14 kJ · mol−1
- ^ ΔfG°, -704.64 kJ · mol−1
- ^ S°, -139.7 J · K−1 · mol−1
- ^ Cp°, -167. J · K−1 · mol−1
- ^ ΔfH°, -314.43 kJ · mol−1
- ^ ΔfG°, -202.87 kJ · mol−1
- ^ S°, 94.6 J · K−1 · mol−1
- ^ Cp°, 84.1 J · K−1 · mol−1
- ^ ΔfH°, -299.66 kJ · mol−1
- ^ ΔfG°, -210.52 kJ · mol−1
- ^ S°, 169.9 J · K−1 · mol−1
- ^ Cp°, -56.5 J · K−1 · mol−1