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3NaHCO3 + H3PO4 → Na3PO4 + 3H2CO3

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
  1. 1Reaction data
  2. 2Thermodynamic changes
  3. 3References
  4. 4Related reactions
  5. 5Related categories

Reaction data

Chemical equation

General equation

Oxidation state of each atom

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
NaHCO3Sodium hydrogencarbonate3
Brønsted base
Salt of volatile acid
H3PO4Phosphoric acid1
Brønsted acid
Nonvolatile acid

Products

Chemical formulaNameCoefficientTypeType in general
equation
Na3PO4Sodium phosphate1
Conjugate base
Salt of non volatile acid
H2CO3Carbonic acid3
Conjugate acid
Volatile acid

Thermodynamic changes

Changes in standard condition (1)

Reaction of sodium hydrogencarbonate and phosphoric acid
ΔrG14.8 kJ/mol
K0.26 × 10−2
pK2.59
3NaHCO3Ionized aqueous solution + H3PO4Un-ionized aqueous solution
Na3PO4Ionized aqueous solution + 3H2CO3Un-ionized aqueous solution
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
−12.214.8−89.9
−4.074.93−30.0
per 1 mol of
−12.214.8−89.9
per 1 mol of
−12.214.8−89.9
per 1 mol of
−4.074.93−30.0

Changes in standard condition (2)

Reaction of sodium hydrogencarbonate and phosphoric acid
ΔrG−109.1 kJ/mol
K1.30 × 1019
pK−19.11
3NaHCO3Ionized aqueous solution + H3PO4Ionized aqueous solution
Na3PO4Ionized aqueous solution + 3H2CO3Un-ionized aqueous solution
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
−23.1−109.1288.6
−7.70−36.3796.20
per 1 mol of
−23.1−109.1288.6
per 1 mol of
−23.1−109.1288.6
per 1 mol of
−7.70−36.3796.20

Changes in standard condition (3)

Reaction of sodium hydrogencarbonate and phosphoric acid
ΔrG14.8 kJ/mol
K0.26 × 10−2
pK2.59
3NaHCO3Ionized aqueous solution + H3PO4Un-ionized aqueous solution
Na3PO4Ionized aqueous solution + 3H2CO3Un-ionized aqueous solution
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
−12.214.8−89.9
−4.074.93−30.0
per 1 mol of
−12.214.8−89.9
per 1 mol of
−12.214.8−89.9
per 1 mol of
−4.074.93−30.0

Changes in standard condition (4)

Reaction of sodium hydrogencarbonate and phosphoric acid
ΔrG17.9 kJ/mol
K0.73 × 10−3
pK3.14
3NaHCO3Un-ionized aqueous solution + H3PO4Un-ionized aqueous solution
Na3PO4Ionized aqueous solution + 3H2CO3Un-ionized aqueous solution
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
23.217.919.3
7.735.976.43
per 1 mol of
23.217.919.3
per 1 mol of
23.217.919.3
per 1 mol of
7.735.976.43

Changes in standard condition (5)

Reaction of sodium hydrogencarbonate and phosphoric acid
ΔrG−105.9 kJ/mol
K3.57 × 1018
pK−18.55
3NaHCO3Un-ionized aqueous solution + H3PO4Ionized aqueous solution
Na3PO4Ionized aqueous solution + 3H2CO3Un-ionized aqueous solution
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
12.3−105.9397.8
4.10−35.30132.6
per 1 mol of
12.3−105.9397.8
per 1 mol of
12.3−105.9397.8
per 1 mol of
4.10−35.30132.6

Changes in standard condition (6)

Reaction of sodium hydrogencarbonate and phosphoric acid
ΔrG17.9 kJ/mol
K0.73 × 10−3
pK3.14
3NaHCO3Un-ionized aqueous solution + H3PO4Un-ionized aqueous solution
Na3PO4Ionized aqueous solution + 3H2CO3Un-ionized aqueous solution
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
23.217.919.3
7.735.976.43
per 1 mol of
23.217.919.3
per 1 mol of
23.217.919.3
per 1 mol of
7.735.976.43

Thermodynamic data of reactants

Chemical formulaStandard 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 formulaStandard 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

  1. 1