Na2SO3 + H3PO4 🔥→ Na2HPO4 + SO2↑ + H2O
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The reaction of sodium sulfite and phosphoric acid yields sodium hydrogenphosphate, sulfur dioxide, and water (Other reactions are here). This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of sodium sulfite and phosphoric acid
General equation
- Salt of volatile acidBrønsted base + Nonvolatile acidBrønsted acid ⟶ Salt of non volatile acidConjugate base + Volatile acidic oxide + H2OConjugate acid
Oxidation state of each atom
- Reaction of sodium sulfite and phosphoric acid
Reactants
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
Na2SO3 | Sodium sulfite | 1 | Brønsted base | Salt of volatile acid |
H3PO4 | Phosphoric acid | 1 | Brønsted acid | Nonvolatile acid |
Products
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
Na2HPO4 | Sodium hydrogenphosphate | 1 | Conjugate base | Salt of non volatile acid |
SO2 | Sulfur dioxide | 1 | – | Volatile acidic oxide |
H2O | Water | 1 | Conjugate acid | Water |
Thermodynamic changes
Changes in standard condition
- Reaction of sodium sulfite and phosphoric acid◆
ΔrG −13.9 kJ/mol K 2.72 × 102 pK −2.44
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 | 49.0 | −13.9 | 212.19 | 24.16 |
per 1 mol of | 49.0 | −13.9 | 212.19 | 24.16 |
per 1 mol of | 49.0 | −13.9 | 212.19 | 24.16 |
per 1 mol of | 49.0 | −13.9 | 212.19 | 24.16 |
per 1 mol of | 49.0 | −13.9 | 212.19 | 24.16 |
per 1 mol of | 49.0 | −13.9 | 212.19 | 24.16 |
Changes in aqueous solution (1)
- Reaction of sodium sulfite and phosphoric acid◆
ΔrG 2.63 kJ/mol K 0.35 × 100 pK 0.46
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 | 49.17 | 2.63 | 156.5 | – |
per 1 mol of | 49.17 | 2.63 | 156.5 | – |
per 1 mol of | 49.17 | 2.63 | 156.5 | – |
per 1 mol of | 49.17 | 2.63 | 156.5 | – |
per 1 mol of | 49.17 | 2.63 | 156.5 | – |
per 1 mol of | 49.17 | 2.63 | 156.5 | – |
Changes in aqueous solution (2)
- Reaction of sodium sulfite and phosphoric acid◆
ΔrG 2.14 kJ/mol K 0.42 × 100 pK 0.37
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 | 23.02 | 2.14 | 70.2 | – |
per 1 mol of | 23.02 | 2.14 | 70.2 | – |
per 1 mol of | 23.02 | 2.14 | 70.2 | – |
per 1 mol of | 23.02 | 2.14 | 70.2 | – |
per 1 mol of | 23.02 | 2.14 | 70.2 | – |
per 1 mol of | 23.02 | 2.14 | 70.2 | – |
Changes in aqueous solution (3)
- Reaction of sodium sulfite and phosphoric acid◆
ΔrG −121.2 kJ/mol K 1.71 × 1021 pK −21.23
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 | 38.2 | −121.2 | 535.0 | – |
per 1 mol of | 38.2 | −121.2 | 535.0 | – |
per 1 mol of | 38.2 | −121.2 | 535.0 | – |
per 1 mol of | 38.2 | −121.2 | 535.0 | – |
per 1 mol of | 38.2 | −121.2 | 535.0 | – |
per 1 mol of | 38.2 | −121.2 | 535.0 | – |
Changes in aqueous solution (4)
- Reaction of sodium sulfite and phosphoric acid◆
ΔrG −121.7 kJ/mol K 2.09 × 1021 pK −21.32
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 | 12.1 | −121.7 | 448.7 | – |
per 1 mol of | 12.1 | −121.7 | 448.7 | – |
per 1 mol of | 12.1 | −121.7 | 448.7 | – |
per 1 mol of | 12.1 | −121.7 | 448.7 | – |
per 1 mol of | 12.1 | −121.7 | 448.7 | – |
per 1 mol of | 12.1 | −121.7 | 448.7 | – |
Changes in aqueous solution (5)
- Reaction of sodium sulfite and phosphoric acid◆
ΔrG 2.63 kJ/mol K 0.35 × 100 pK 0.46
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 | 49.17 | 2.63 | 156.5 | – |
per 1 mol of | 49.17 | 2.63 | 156.5 | – |
per 1 mol of | 49.17 | 2.63 | 156.5 | – |
per 1 mol of | 49.17 | 2.63 | 156.5 | – |
per 1 mol of | 49.17 | 2.63 | 156.5 | – |
per 1 mol of | 49.17 | 2.63 | 156.5 | – |
Changes in aqueous solution (6)
- Reaction of sodium sulfite and phosphoric acid◆
ΔrG 2.14 kJ/mol K 0.42 × 100 pK 0.37
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 | 23.02 | 2.14 | 70.2 | – |
per 1 mol of | 23.02 | 2.14 | 70.2 | – |
per 1 mol of | 23.02 | 2.14 | 70.2 | – |
per 1 mol of | 23.02 | 2.14 | 70.2 | – |
per 1 mol of | 23.02 | 2.14 | 70.2 | – |
per 1 mol of | 23.02 | 2.14 | 70.2 | – |
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 |
---|---|---|---|---|
Na2SO3 (cr) | -1100.8[1] | -1012.5[1] | 145.94[1] | 120.25[1] |
Na2SO3 (ai) | -1115.87[1] | -1010.39[1] | 87.9[1] | – |
Na2SO3 (cr) 7 hydrate | -3162.3[1] | -2676.1[1] | 444[1] | – |
H3PO4 (cr) | -1279.0[1] | -1119.1[1] | 110.50[1] | 106.06[1] |
H3PO4 (l) | -1266.9[1] | – | – | – |
H3PO4 (ai) | -1277.4[1] | -1018.7[1] | -220.3[1] | – |
H3PO4 (ao) | -1288.34[1] | -1142.54[1] | 158.2[1] | – |
H3PO4 (cr) 0.5 hydrate | -1431.3[1] | -1242.1[1] | 129.16[1] | 126.02[1] |
H3PO4 (cr) 1 hydrate | -1568.83[1] | – | – | – |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (l):Liquid, (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 |
---|---|---|---|---|
Na2HPO4 (cr) | -1748.1[1] | -1608.2[1] | 150.50[1] | 135.31[1] |
Na2HPO4 (ai) | -1772.38[1] | -1612.98[1] | 84.5[1] | – |
Na2HPO4 (cr) 2 hydrate | -2346.0[1] | -2088.5[1] | 221.3[1] | – |
Na2HPO4 (cr) 7 hydrate | -3821.7[1] | -3279.8[1] | 434.59[1] | – |
Na2HPO4 (cr) 12 hydrate | -5297.8[1] | -4467.8[1] | 633.83[1] | – |
SO2 (l) | -320.5[1] | – | – | – |
SO2 (g) | -296.830[1] | -300.194[1] | 248.22[1] | 39.87[1] |
SO2 (ao) | -322.980[1] | -300.676[1] | 161.9[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, (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°, -1100.8 kJ · mol−1
- ^ ΔfG°, -1012.5 kJ · mol−1
- ^ S°, 145.94 J · K−1 · mol−1
- ^ Cp°, 120.25 J · K−1 · mol−1
- ^ ΔfH°, -1115.87 kJ · mol−1
- ^ ΔfG°, -1010.39 kJ · mol−1
- ^ S°, 87.9 J · K−1 · mol−1
- ^ ΔfH°, -3162.3 kJ · mol−1
- ^ ΔfG°, -2676.1 kJ · mol−1
- ^ S°, 444. J · K−1 · mol−1
- ^ ΔfH°, -1279.0 kJ · mol−1
- ^ ΔfG°, -1119.1 kJ · mol−1
- ^ S°, 110.50 J · K−1 · mol−1
- ^ Cp°, 106.06 J · K−1 · mol−1
- ^ ΔfH°, -1266.9 kJ · mol−1
- ^ ΔfH°, -1277.4 kJ · mol−1
- ^ ΔfG°, -1018.7 kJ · mol−1
- ^ S°, -220.3 J · K−1 · mol−1
- ^ ΔfH°, -1288.34 kJ · mol−1
- ^ ΔfG°, -1142.54 kJ · mol−1
- ^ S°, 158.2 J · K−1 · mol−1
- ^ ΔfH°, -1431.3 kJ · mol−1
- ^ ΔfG°, -1242.1 kJ · mol−1
- ^ S°, 129.16 J · K−1 · mol−1
- ^ Cp°, 126.02 J · K−1 · mol−1
- ^ ΔfH°, -1568.83 kJ · mol−1
- ^ ΔfH°, -1748.1 kJ · mol−1
- ^ ΔfG°, -1608.2 kJ · mol−1
- ^ S°, 150.50 J · K−1 · mol−1
- ^ Cp°, 135.31 J · K−1 · mol−1
- ^ ΔfH°, -1772.38 kJ · mol−1
- ^ ΔfG°, -1612.98 kJ · mol−1
- ^ S°, 84.5 J · K−1 · mol−1
- ^ ΔfH°, -2346.0 kJ · mol−1
- ^ ΔfG°, -2088.5 kJ · mol−1
- ^ S°, 221.3 J · K−1 · mol−1
- ^ ΔfH°, -3821.7 kJ · mol−1
- ^ ΔfG°, -3279.8 kJ · mol−1
- ^ S°, 434.59 J · K−1 · mol−1
- ^ ΔfH°, -5297.8 kJ · mol−1
- ^ ΔfG°, -4467.8 kJ · mol−1
- ^ S°, 633.83 J · K−1 · mol−1
- ^ ΔfH°, -320.5 kJ · mol−1
- ^ ΔfH°, -296.830 kJ · mol−1
- ^ ΔfG°, -300.194 kJ · mol−1
- ^ S°, 248.22 J · K−1 · mol−1
- ^ Cp°, 39.87 J · K−1 · mol−1
- ^ ΔfH°, -322.980 kJ · mol−1
- ^ ΔfG°, -300.676 kJ · mol−1
- ^ S°, 161.9 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