NaF + HNO3 → NaNO3 + HF↑
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- Reaction of sodium fluoride and nitric acid
The reaction of sodium fluoride and nitric acid yields sodium nitrate and hydrogen fluoride. This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of sodium fluoride and nitric acid
General equation
- Salt of weak acidBrønsted base + Strong acidBrønsted acid ⟶ Salt of strong acidConjugate base + Weak acidConjugate acid
Oxidation state of each atom
- Reaction of sodium fluoride and nitric acid
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| NaF | Sodium fluoride | 1 | Brønsted base | Salt of weak acid |
| HNO3 | Nitric acid | 1 | Brønsted acid | Strong acid |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| NaNO3 | Sodium nitrate | 1 | Conjugate base | Salt of strong acid |
| HF | Hydrogen fluoride | 1 | Conjugate acid | Weak acid |
Thermodynamic changes
Changes in standard condition
- Reaction of sodium fluoride and nitric acid◆
ΔrG −16.0 kJ/mol K 6.35 × 102 pK −2.80
| 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 | 8.8 | −16.0 | 83.24 | −34.72 |
per 1 mol of | 8.8 | −16.0 | 83.24 | −34.72 |
per 1 mol of | 8.8 | −16.0 | 83.24 | −34.72 |
per 1 mol of | 8.8 | −16.0 | 83.24 | −34.72 |
per 1 mol of | 8.8 | −16.0 | 83.24 | −34.72 |
Changes in aqueous solution (1)
- Reaction of sodium fluoride and nitric acid◆
ΔrG 5.6 kJ/mol K 0.10 × 100 pK 0.98
| 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 | 61.5 | 5.6 | 187.6 | 135.7 |
per 1 mol of | 61.5 | 5.6 | 187.6 | 135.7 |
per 1 mol of | 61.5 | 5.6 | 187.6 | 135.7 |
per 1 mol of | 61.5 | 5.6 | 187.6 | 135.7 |
per 1 mol of | 61.5 | 5.6 | 187.6 | 135.7 |
Changes in aqueous solution (2)
- Reaction of sodium fluoride and nitric acid◆
ΔrG −18.04 kJ/mol K 1.45 × 103 pK −3.16
| 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 | 12.55 | −18.04 | 102.5 | – |
per 1 mol of | 12.55 | −18.04 | 102.5 | – |
per 1 mol of | 12.55 | −18.04 | 102.5 | – |
per 1 mol of | 12.55 | −18.04 | 102.5 | – |
per 1 mol of | 12.55 | −18.04 | 102.5 | – |
Changes in aqueous solution (3)
- Reaction of sodium fluoride and nitric acid◆
ΔrG −18.04 kJ/mol K 1.45 × 103 pK −3.16
| 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 | 12.55 | −18.04 | 102.5 | – |
per 1 mol of | 12.55 | −18.04 | 102.5 | – |
per 1 mol of | 12.55 | −18.04 | 102.5 | – |
per 1 mol of | 12.55 | −18.04 | 102.5 | – |
per 1 mol of | 12.55 | −18.04 | 102.5 | – |
Changes in aqueous solution (4)
- Reaction of sodium fluoride and nitric acid◆
ΔrG −0.01 kJ/mol K 1.00 × 100 pK −0.00
| 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 | 0.00 | −0.01 | 0.0 | −0.1 |
per 1 mol of | 0.00 | −0.0100 | 0.0 | −0.10 |
per 1 mol of | 0.00 | −0.0100 | 0.0 | −0.10 |
per 1 mol of | 0.00 | −0.0100 | 0.0 | −0.10 |
per 1 mol of | 0.00 | −0.0100 | 0.0 | −0.10 |
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 |
|---|---|---|---|---|
| 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] |
| HNO3 (l) | -174.10[1] | -80.71[1] | 155.60[1] | 109.87[1] |
| HNO3 (g) | -135.06[1] | -74.72[1] | 266.38[1] | 53.35[1] |
| HNO3 (ai) | -207.36[1] | -111.25[1] | 146.4[1] | -86.6[1] |
| HNO3 (l) 1 hydrate | -473.46[1] | -328.77[1] | 216.90[1] | 182.46[1] |
| HNO3 (l) 3 hydrate | -1056.04[1] | -811.09[1] | 346.98[1] | 325.14[1] |
* (cr):Crystalline solid, (g):Gas, (ai):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 |
|---|---|---|---|---|
| NaNO3 (cr) | -467.85[1] | -367.00[1] | 116.52[1] | 92.88[1] |
| NaNO3 (ai) | -447.48[1] | -373.15[1] | 205.4[1] | -40.2[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°, -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°, -174.10 kJ · mol−1
- ^ ΔfG°, -80.71 kJ · mol−1
- ^ S°, 155.60 J · K−1 · mol−1
- ^ Cp°, 109.87 J · K−1 · mol−1
- ^ ΔfH°, -135.06 kJ · mol−1
- ^ ΔfG°, -74.72 kJ · mol−1
- ^ S°, 266.38 J · K−1 · mol−1
- ^ Cp°, 53.35 J · K−1 · mol−1
- ^ ΔfH°, -207.36 kJ · mol−1
- ^ ΔfG°, -111.25 kJ · mol−1
- ^ S°, 146.4 J · K−1 · mol−1
- ^ Cp°, -86.6 J · K−1 · mol−1
- ^ ΔfH°, -473.46 kJ · mol−1
- ^ ΔfG°, -328.77 kJ · mol−1
- ^ S°, 216.90 J · K−1 · mol−1
- ^ Cp°, 182.46 J · K−1 · mol−1
- ^ ΔfH°, -1056.04 kJ · mol−1
- ^ ΔfG°, -811.09 kJ · mol−1
- ^ S°, 346.98 J · K−1 · mol−1
- ^ Cp°, 325.14 J · K−1 · mol−1
- ^ ΔfH°, -467.85 kJ · mol−1
- ^ ΔfG°, -367.00 kJ · mol−1
- ^ S°, 116.52 J · K−1 · mol−1
- ^ Cp°, 92.88 J · K−1 · mol−1
- ^ ΔfH°, -447.48 kJ · mol−1
- ^ ΔfG°, -373.15 kJ · mol−1
- ^ S°, 205.4 J · K−1 · mol−1
- ^ Cp°, -40.2 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