NH4F + LiOH → LiF↓ + NH3↑ + H2O
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- Reaction of ammonium fluoride and lithium hydroxide
The reaction of ammonium fluoride and lithium hydroxide yields lithium fluoride, ammonia, and water. This reaction is an acid-base reaction and is classified as follows:
- Reaction of salt of weak base and strong base
- Reaction of volatile acid and non volatile base
- Precipitation reaction
Table of contents
Reaction data
Chemical equation
- Reaction of ammonium fluoride and lithium 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)
- Reaction of volatile acid and non volatile base
- Salt of volatile baseBrønsted acid + Nonvolatile baseBrønsted base ⟶ Salt of non volatile baseConjugate acid + Volatile 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 ammonium fluoride and lithium hydroxide
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| NH4F | Ammonium fluoride | 1 | Brønsted acid Lewis acid | Salt of weak base Salt of volatile base Very soluble in water |
| LiOH | Lithium hydroxide | 1 | Brønsted base Lewis base | Strong base Nonvolatile base Soluble in water |
Products
Thermodynamic changes
Changes in standard condition
- Reaction of ammonium fluoride and lithium hydroxide◆
ΔrG −53.66 kJ/mol K 2.52 × 109 pK −9.40
| 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 | 0.98 | −53.66 | 183.25 | 37.01 |
per 1 mol of | 0.980 | −53.66 | 183.25 | 37.01 |
per 1 mol of | 0.980 | −53.66 | 183.25 | 37.01 |
per 1 mol of | 0.980 | −53.66 | 183.25 | 37.01 |
per 1 mol of | 0.980 | −53.66 | 183.25 | 37.01 |
per 1 mol of | 0.980 | −53.66 | 183.25 | 37.01 |
Changes in aqueous solution (1)
- Reaction of ammonium fluoride and lithium hydroxide◆
ΔrG −32.62 kJ/mol K 5.19 × 105 pK −5.71
| 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 | 25.71 | −32.62 | 195.6 | 258.6 |
per 1 mol of | 25.71 | −32.62 | 195.6 | 258.6 |
per 1 mol of | 25.71 | −32.62 | 195.6 | 258.6 |
per 1 mol of | 25.71 | −32.62 | 195.6 | 258.6 |
per 1 mol of | 25.71 | −32.62 | 195.6 | 258.6 |
per 1 mol of | 25.71 | −32.62 | 195.6 | 258.6 |
Changes in aqueous solution (2)
- Reaction of ammonium fluoride and lithium hydroxide◆
ΔrG −42.67 kJ/mol K 2.99 × 107 pK −7.48
| 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 | −8.47 | −42.67 | 114.5 | – |
per 1 mol of | −8.47 | −42.67 | 114.5 | – |
per 1 mol of | −8.47 | −42.67 | 114.5 | – |
per 1 mol of | −8.47 | −42.67 | 114.5 | – |
per 1 mol of | −8.47 | −42.67 | 114.5 | – |
per 1 mol of | −8.47 | −42.67 | 114.5 | – |
Changes in aqueous solution (3)
- Reaction of ammonium fluoride and lithium hydroxide◆
ΔrG −31.4 kJ/mol K 3.17 × 105 pK −5.50
| 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 | 25.6 | −31.4 | 191.3 | – |
per 1 mol of | 25.6 | −31.4 | 191.3 | – |
per 1 mol of | 25.6 | −31.4 | 191.3 | – |
per 1 mol of | 25.6 | −31.4 | 191.3 | – |
per 1 mol of | 25.6 | −31.4 | 191.3 | – |
per 1 mol of | 25.6 | −31.4 | 191.3 | – |
Changes in aqueous solution (4)
- Reaction of ammonium fluoride and lithium hydroxide◆
ΔrG −41.4 kJ/mol K 1.79 × 107 pK −7.25
| 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 | −8.6 | −41.4 | 110.2 | – |
per 1 mol of | −8.6 | −41.4 | 110.2 | – |
per 1 mol of | −8.6 | −41.4 | 110.2 | – |
per 1 mol of | −8.6 | −41.4 | 110.2 | – |
per 1 mol of | −8.6 | −41.4 | 110.2 | – |
per 1 mol of | −8.6 | −41.4 | 110.2 | – |
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 |
|---|---|---|---|---|
| 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] |
| LiOH (cr) | -484.93[1] | -438.95[1] | 42.80[1] | 49.66[1] |
| LiOH (g) | -238.1[1] | -242.3[1] | 210.90[1] | 46.02[1] |
| LiOH (ai) | -508.48[1] | -450.58[1] | 2.80[1] | -79.9[1] |
| LiOH (ao) | -508.4[1] | -451.8[1] | 7.1[1] | – |
| LiOH (cr) 1 hydrate | -788.01[1] | -680.95[1] | 71.21[1] | 79.50[1] |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (g):Gas, (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 |
|---|---|---|---|---|
| LiF (cr) | -615.97[1] | -587.71[1] | 35.65[1] | 41.59[1] |
| LiF (g) | -339.82[1] | -360.64[1] | 200.297[1] | 31.30[1] |
| LiF (ai) | -611.12[1] | -571.9[1] | -0.4[1] | -38.07[1] |
| NH3 (g) | -46.11[1] | -16.45[1] | 192.45[1] | 35.06[1] |
| NH3 (ao) | -80.29[1] | -26.50[1] | 111.3[1] | – |
| H2O (cr) | – | – | – | – |
| H2O (l) | -285.830[1] | -237.129[1] | 69.91[1] | 75.291[1] |
| H2O (g) | -241.818[1] | -228.572[1] | 188.825[1] | 33.577[1] |
* (cr):Crystalline solid, (g):Gas, (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution, (l):Liquid
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°, -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°, -484.93 kJ · mol−1
- ^ ΔfG°, -438.95 kJ · mol−1
- ^ S°, 42.80 J · K−1 · mol−1
- ^ Cp°, 49.66 J · K−1 · mol−1
- ^ ΔfH°, -238.1 kJ · mol−1
- ^ ΔfG°, -242.3 kJ · mol−1
- ^ S°, 210.90 J · K−1 · mol−1
- ^ Cp°, 46.02 J · K−1 · mol−1
- ^ ΔfH°, -508.48 kJ · mol−1
- ^ ΔfG°, -450.58 kJ · mol−1
- ^ S°, 2.80 J · K−1 · mol−1
- ^ Cp°, -79.9 J · K−1 · mol−1
- ^ ΔfH°, -508.4 kJ · mol−1
- ^ ΔfG°, -451.8 kJ · mol−1
- ^ S°, 7.1 J · K−1 · mol−1
- ^ ΔfH°, -788.01 kJ · mol−1
- ^ ΔfG°, -680.95 kJ · mol−1
- ^ S°, 71.21 J · K−1 · mol−1
- ^ Cp°, 79.50 J · K−1 · mol−1
- ^ ΔfH°, -615.97 kJ · mol−1
- ^ ΔfG°, -587.71 kJ · mol−1
- ^ S°, 35.65 J · K−1 · mol−1
- ^ Cp°, 41.59 J · K−1 · mol−1
- ^ ΔfH°, -339.82 kJ · mol−1
- ^ ΔfG°, -360.64 kJ · mol−1
- ^ S°, 200.297 J · K−1 · mol−1
- ^ Cp°, 31.30 J · K−1 · mol−1
- ^ ΔfH°, -611.12 kJ · mol−1
- ^ ΔfG°, -571.9 kJ · mol−1
- ^ S°, -0.4 J · K−1 · mol−1
- ^ Cp°, -38.07 J · K−1 · mol−1
- ^ ΔfH°, -46.11 kJ · mol−1
- ^ ΔfG°, -16.45 kJ · mol−1
- ^ S°, 192.45 J · K−1 · mol−1
- ^ Cp°, 35.06 J · K−1 · mol−1
- ^ ΔfH°, -80.29 kJ · mol−1
- ^ ΔfG°, -26.50 kJ · mol−1
- ^ S°, 111.3 J · K−1 · mol−1
- ^ ΔfH°, -285.830 kJ · mol−1
- ^ ΔfG°, -237.129 kJ · mol−1
- ^ S°, 69.91 J · K−1 · mol−1
- ^ Cp°, 75.291 J · K−1 · mol−1
- ^ ΔfH°, -241.818 kJ · mol−1
- ^ ΔfG°, -228.572 kJ · mol−1
- ^ S°, 188.825 J · K−1 · mol−1
- ^ Cp°, 33.577 J · K−1 · mol−1