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Na3PO4 + 2H2CO3 → NaH2PO4 + 2NaHCO3

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Reaction of sodium phosphate and carbonic acid
Na3PO4Sodium phosphate + 2H2CO3Carbonic acid
⟶
NaH2PO4Sodium dihydrogenphosphate + 2NaHCO3Sodium hydrogencarbonate

The reaction of sodium phosphate and carbonic acid yields sodium dihydrogenphosphate and sodium hydrogencarbonate (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

Reaction of sodium phosphate and carbonic acid
Na3PO4Sodium phosphate + 2H2CO3Carbonic acid
⟶
NaH2PO4Sodium dihydrogenphosphate + 2NaHCO3Sodium hydrogencarbonate

General equation

Reaction of salt and acid with generating acid salt
SaltBrønsted base + AcidBrønsted acid
⟶
Acid saltConjugate acid base

Oxidation state of each atom

Reaction of sodium phosphate and carbonic acid

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
Na3PO4Sodium phosphate1
Brønsted base
Salt
H2CO3Carbonic acid2
Brønsted acid
Acid

Products

Chemical formulaNameCoefficientTypeType in general
equation
NaH2PO4Sodium dihydrogenphosphate1
Conjugate acid base
Acid salt
NaHCO3Sodium hydrogencarbonate2
Conjugate acid base
Acid salt

Thermodynamic changes

Changes in standard condition (1)

Reaction of sodium phosphate and carbonic acid
◆
ΔrG−38.8 kJ/mol
K6.27 × 106
pK−6.80
Na3PO4Ionized aqueous solution + 2H2CO3Un-ionized aqueous solution
⟶
NaH2PO4Ionized aqueous solution + 2NaHCO3Ionized 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
−3.4−38.8118.3–
per 1 mol of
−3.4−38.8118.3–
per 1 mol of
−1.7−19.459.15–
−3.4−38.8118.3–
−1.7−19.459.15–

Changes in standard condition (2)

Reaction of sodium phosphate and carbonic acid
◆
ΔrG−40.9 kJ/mol
K1.46 × 107
pK−7.17
Na3PO4Ionized aqueous solution + 2H2CO3Un-ionized aqueous solution
⟶
NaH2PO4Ionized aqueous solution + 2NaHCO3Un-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
−27.0−40.945.5–
per 1 mol of
−27.0−40.945.5–
per 1 mol of
−13.5−20.422.8–
−27.0−40.945.5–
−13.5−20.422.8–

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
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

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
NaH2PO4 (cr)-1536.8[1]-1386.1[1]127.49[1]116.86[1]
NaH2PO4 (ai)-1536.41[1]-1392.17[1]149.4[1]–
NaH2PO4 (cr)
1 hydrate
-1833.0[1]–––
NaH2PO4 (cr)
2 hydrate
-2128.4[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]–
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution

References

List of references

  1. 1
    Janiel J. Reed (1989)
    The NBS Tables of Chemical Thermodynamic Properties: Selected Values for Inorganic and C1 and C2 Organic Substances in SI Units
    National Institute of Standards and Technology (NIST)