3NaHCO3 + H3PO4 → Na3PO4 + 3H2CO3
Last updated:
The reaction of sodium hydrogencarbonate and phosphoric acid yields sodium phosphate and carbonic acid (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 hydrogencarbonate and phosphoric acid
General equation
- Salt of volatile acidBrønsted base + Nonvolatile acidBrønsted acid ⟶ Salt of non volatile acidConjugate base + Volatile acidConjugate acid
Oxidation state of each atom
- Reaction of sodium hydrogencarbonate and phosphoric acid
Reactants
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
NaHCO3 | Sodium hydrogencarbonate | 3 | Brønsted base | Salt of volatile acid |
H3PO4 | Phosphoric acid | 1 | Brønsted acid | Nonvolatile acid |
Products
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
Na3PO4 | Sodium phosphate | 1 | Conjugate base | Salt of non volatile acid |
H2CO3 | Carbonic acid | 3 | Conjugate acid | Volatile acid |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of sodium hydrogencarbonate and phosphoric acid◆
ΔrG 14.8 kJ/mol K 0.26 × 10−2 pK 2.59
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 | −12.2 | 14.8 | −89.9 | – |
per 1 mol of | −4.07 | 4.93 | −30.0 | – |
per 1 mol of | −12.2 | 14.8 | −89.9 | – |
per 1 mol of | −12.2 | 14.8 | −89.9 | – |
per 1 mol of | −4.07 | 4.93 | −30.0 | – |
Changes in standard condition (2)
- Reaction of sodium hydrogencarbonate and phosphoric acid◆
ΔrG −109.1 kJ/mol K 1.30 × 1019 pK −19.11
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 | −23.1 | −109.1 | 288.6 | – |
per 1 mol of | −7.70 | −36.37 | 96.20 | – |
per 1 mol of | −23.1 | −109.1 | 288.6 | – |
per 1 mol of | −23.1 | −109.1 | 288.6 | – |
per 1 mol of | −7.70 | −36.37 | 96.20 | – |
Changes in standard condition (3)
- Reaction of sodium hydrogencarbonate and phosphoric acid◆
ΔrG 14.8 kJ/mol K 0.26 × 10−2 pK 2.59
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 | −12.2 | 14.8 | −89.9 | – |
per 1 mol of | −4.07 | 4.93 | −30.0 | – |
per 1 mol of | −12.2 | 14.8 | −89.9 | – |
per 1 mol of | −12.2 | 14.8 | −89.9 | – |
per 1 mol of | −4.07 | 4.93 | −30.0 | – |
Changes in standard condition (4)
- Reaction of sodium hydrogencarbonate and phosphoric acid◆
ΔrG 17.9 kJ/mol K 0.73 × 10−3 pK 3.14
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 | 23.2 | 17.9 | 19.3 | – |
per 1 mol of | 7.73 | 5.97 | 6.43 | – |
per 1 mol of | 23.2 | 17.9 | 19.3 | – |
per 1 mol of | 23.2 | 17.9 | 19.3 | – |
per 1 mol of | 7.73 | 5.97 | 6.43 | – |
Changes in standard condition (5)
- Reaction of sodium hydrogencarbonate and phosphoric acid◆
ΔrG −105.9 kJ/mol K 3.57 × 1018 pK −18.55
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 | 12.3 | −105.9 | 397.8 | – |
per 1 mol of | 4.10 | −35.30 | 132.6 | – |
per 1 mol of | 12.3 | −105.9 | 397.8 | – |
per 1 mol of | 12.3 | −105.9 | 397.8 | – |
per 1 mol of | 4.10 | −35.30 | 132.6 | – |
Changes in standard condition (6)
- Reaction of sodium hydrogencarbonate and phosphoric acid◆
ΔrG 17.9 kJ/mol K 0.73 × 10−3 pK 3.14
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 | 23.2 | 17.9 | 19.3 | – |
per 1 mol of | 7.73 | 5.97 | 6.43 | – |
per 1 mol of | 23.2 | 17.9 | 19.3 | – |
per 1 mol of | 23.2 | 17.9 | 19.3 | – |
per 1 mol of | 7.73 | 5.97 | 6.43 | – |
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 |
---|---|---|---|---|
NaHCO3 (cr) | -950.81[1] | -851.0[1] | 101.7[1] | 87.61[1] |
NaHCO3 (ai) | -932.11[1] | -848.66[1] | 150.2[1] | – |
NaHCO3 (ao) | -943.9[1] | -849.7[1] | 113.8[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, (ao):Un-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 |
---|---|---|---|---|
Na3PO4 (cr) | -1917.40[1] | -1788.80[1] | 173.80[1] | 153.47[1] |
Na3PO4 (ai) | -1997.9[1] | -1804.5[1] | -43.3[1] | – |
H2CO3 (ao) | -699.65[1] | -623.08[1] | 187.4[1] | – |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (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°, -950.81 kJ · mol−1
- ^ ΔfG°, -851.0 kJ · mol−1
- ^ S°, 101.7 J · K−1 · mol−1
- ^ Cp°, 87.61 J · K−1 · mol−1
- ^ ΔfH°, -932.11 kJ · mol−1
- ^ ΔfG°, -848.66 kJ · mol−1
- ^ S°, 150.2 J · K−1 · mol−1
- ^ ΔfH°, -943.9 kJ · mol−1
- ^ ΔfG°, -849.7 kJ · mol−1
- ^ S°, 113.8 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°, -1917.40 kJ · mol−1
- ^ ΔfG°, -1788.80 kJ · mol−1
- ^ S°, 173.80 J · K−1 · mol−1
- ^ Cp°, 153.47 J · K−1 · mol−1
- ^ ΔfH°, -1997.9 kJ · mol−1
- ^ ΔfG°, -1804.5 kJ · mol−1
- ^ S°, -43.3 J · K−1 · mol−1
- ^ ΔfH°, -699.65 kJ · mol−1
- ^ ΔfG°, -623.08 kJ · mol−1
- ^ S°, 187.4 J · K−1 · mol−1