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(NH4)2CO3 + NaOH → NaHCO3 + 2NH3↑ + H2O

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Reaction of ammonium carbonate and sodium hydroxide
(NH4)2CO3Ammonium carbonate + NaOHSodium hydroxide
⟶
NaHCO3Sodium hydrogencarbonate + 2NH3↑Ammonia + H2OWater

The reaction of ammonium carbonate and sodium hydroxide yields sodium hydrogencarbonate, ammonia, and water (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 ammonium carbonate and sodium hydroxide
(NH4)2CO3Ammonium carbonate + NaOHSodium hydroxide
⟶
NaHCO3Sodium hydrogencarbonate + 2NH3↑Ammonia + H2OWater

General equation

Reaction of salt of weak base and strong base
Salt of weak baseBrønsted acid + Strong baseBrønsted base
⟶
Salt of strong baseConjugate acid + Weak baseConjugate base + (H2O)
Reaction of volatile acid and non volatile base
Salt of volatile baseBrønsted acid + Nonvolatile baseBrønsted base
⟶
Salt of non volatile baseConjugate acid + Volatile baseConjugate base + (H2O)

Oxidation state of each atom

Reaction of ammonium carbonate and sodium hydroxide

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
(NH4)2CO3Ammonium carbonate1
Brønsted acid
Salt of weak base
Salt of volatile base
NaOHSodium hydroxide1
Brønsted base
Strong base
Nonvolatile base

Products

Chemical formulaNameCoefficientTypeType in general
equation
NaHCO3Sodium hydrogencarbonate1
Conjugate acid
Salt of strong base
Salt of non volatile base
NH3Ammonia2
Conjugate base
Weak base
Volatile base
H2OWater1
–
Water

Thermodynamic changes

Changes in aqueous solution (1)

Reaction of ammonium carbonate and sodium hydroxide
◆
ΔrG−13.12 kJ/mol
K1.99 × 102
pK−2.30
(NH4)2CO3Ionized aqueous solution + NaOHIonized aqueous solution
⟶
NaHCO3Ionized aqueous solution + 2NH3↑Gas + H2OLiquid
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
102.10−13.12387.0–
per 1 mol of
102.10−13.12387.0–
per 1 mol of
102.10−13.12387.0–
102.10−13.12387.0–
per 1 mol of
51.050−6.560193.5–
per 1 mol of
102.10−13.12387.0–

Changes in aqueous solution (2)

Reaction of ammonium carbonate and sodium hydroxide
◆
ΔrG−33.22 kJ/mol
K6.61 × 105
pK−5.82
(NH4)2CO3Ionized aqueous solution + NaOHIonized aqueous solution
⟶
NaHCO3Ionized aqueous solution + 2NH3↑Un-ionized aqueous solution + H2OLiquid
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
33.74−33.22224.7–
per 1 mol of
33.74−33.22224.7–
per 1 mol of
33.74−33.22224.7–
33.74−33.22224.7–
per 1 mol of
16.87−16.61112.3–
per 1 mol of
33.74−33.22224.7–

Changes in aqueous solution (3)

Reaction of ammonium carbonate and sodium hydroxide
◆
ΔrG−14.2 kJ/mol
K3.07 × 102
pK−2.49
(NH4)2CO3Ionized aqueous solution + NaOHIonized aqueous solution
⟶
NaHCO3Un-ionized aqueous solution + 2NH3↑Gas + H2OLiquid
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
90.3−14.2350.6–
per 1 mol of
90.3−14.2350.6–
per 1 mol of
90.3−14.2350.6–
90.3−14.2350.6–
per 1 mol of
45.1−7.10175.3–
per 1 mol of
90.3−14.2350.6–

Changes in aqueous solution (4)

Reaction of ammonium carbonate and sodium hydroxide
◆
ΔrG−34.3 kJ/mol
K1.02 × 106
pK−6.01
(NH4)2CO3Ionized aqueous solution + NaOHIonized aqueous solution
⟶
NaHCO3Un-ionized aqueous solution + 2NH3↑Un-ionized aqueous solution + H2OLiquid
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
22.0−34.3188.3–
per 1 mol of
22.0−34.3188.3–
per 1 mol of
22.0−34.3188.3–
22.0−34.3188.3–
per 1 mol of
11.0−17.194.15–
per 1 mol of
22.0−34.3188.3–

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
(NH4)2CO3 (ai)-942.15[1]-686.42[1]169.9[1]–
NaOH (cr)-425.609[1]-379.494[1]64.455[1]59.54[1]
NaOH (g)-207.1[1]-210.0[1]228.43[1]48.37[1]
NaOH (ai)-470.114[1]-419.150[1]48.1[1]-102.1[1]
NaOH (cr)
1 hydrate
-734.543[1]-629.338[1]99.50[1]90.17[1]
NaOH (l)
2 hydrate
-1019.076[1]-873.091[1]195.979[1]239.41[1]
NaOH (l)
3.5 hydrate
-1459.798[1]-1236.356[1]286.089[1]354.43[1]
NaOH (l)
4 hydrate
-1605.15[1]-1356.64[1]318.70[1]–
NaOH (l)
5 hydrate
-1894.31[1]-1596.34[1]386.06[1]–
NaOH (l)
7 hydrate
-2469.02[1]-2073.80[1]526.31[1]–
* (ai):Ionized aqueous solution, (cr):Crystalline solid, (g):Gas, (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
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]–
NH3 (g)-46.11[1]-16.45[1]192.45[1]35.06[1]
NH3 (ao)-80.29[1]-26.50[1]111.3[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, (ao):Un-ionized aqueous solution, (g):Gas, (l):Liquid

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)