Li2S2O3 + 2NaF 💧→ 2LiF↓ + Na2S2O3
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The reaction of lithium thiosulfate and sodium fluoride yields lithium fluoride and sodium thiosulfate. This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of lithium thiosulfate and sodium 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 lithium thiosulfate and sodium fluoride
Reactants
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
Li2S2O3 | Lithium thiosulfate | 1 | Lewis acid | Soluble in water |
NaF | Sodium fluoride | 2 | Lewis base | Very soluble in water |
Products
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
LiF | Lithium fluoride | 2 | Lewis conjugate | Slightly soluble in water |
Na2S2O3 | Sodium thiosulfate | 1 | Non-redox product | – |
Thermodynamic changes
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 |
---|---|---|---|---|
Li2S2O3 | – | – | – | – |
NaF (cr) | -573.647[1] | -543.494[1] | 51.46[1] | 46.86[1] |
NaF (g) | -291.2[1] | -310.5[1] | 217.59[1] | 34.221[1] |
NaF (ai) | -572.75[1] | -540.68[1] | 45.2[1] | -60.2[1] |
* (cr):Crystalline solid, (g):Gas, (ai):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] |
Na2S2O3 (cr) | -1123.0[1] | -1028.0[1] | 155[1] | – |
Na2S2O3 (ai) | -1132.40[1] | -1046.0[1] | 184.1[1] | – |
Na2S2O3 (cr) 5 hydrate | -2607.93[1] | -2229.8[1] | 372[1] | – |
* (cr):Crystalline solid, (g):Gas, (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°, -573.647 kJ · mol−1
- ^ ΔfG°, -543.494 kJ · mol−1
- ^ S°, 51.46 J · K−1 · mol−1
- ^ Cp°, 46.86 J · K−1 · mol−1
- ^ ΔfH°, -291.2 kJ · mol−1
- ^ ΔfG°, -310.5 kJ · mol−1
- ^ S°, 217.59 J · K−1 · mol−1
- ^ Cp°, 34.221 J · K−1 · mol−1
- ^ ΔfH°, -572.75 kJ · mol−1
- ^ ΔfG°, -540.68 kJ · mol−1
- ^ S°, 45.2 J · K−1 · mol−1
- ^ Cp°, -60.2 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°, -1123.0 kJ · mol−1
- ^ ΔfG°, -1028.0 kJ · mol−1
- ^ S°, 155. J · K−1 · mol−1
- ^ ΔfH°, -1132.40 kJ · mol−1
- ^ ΔfG°, -1046.0 kJ · mol−1
- ^ S°, 184.1 J · K−1 · mol−1
- ^ ΔfH°, -2607.93 kJ · mol−1
- ^ ΔfG°, -2229.8 kJ · mol−1
- ^ S°, 372. J · K−1 · mol−1