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Na2SO3 + 2HCl → 2NaCl + SO2 + H2O

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Reaction of sodium sulfite and hydrogen chloride
Na2SO3Sodium sulfite + 2HClHydrogen chloride
⟶
2NaClSodium chloride + SO2Sulfur dioxide + H2OWater

The reaction of sodium sulfite and hydrogen chloride yields sodium chloride, sulfur dioxide, 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 sodium sulfite and hydrogen chloride
Na2SO3Sodium sulfite + 2HClHydrogen chloride
⟶
2NaClSodium chloride + SO2Sulfur dioxide + H2OWater

General equation

Reaction of salt of weak acid and strong acid with generating weak acidic oxide
Salt of weak acidBrønsted base + Strong acidBrønsted acid
⟶
Salt of strong acidConjugate base + Acidic oxide + H2OConjugate acid

Oxidation state of each atom

Reaction of sodium sulfite and hydrogen chloride

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
Na2SO3Sodium sulfite1
Brønsted base
Salt of weak acid
HClHydrogen chloride2
Brønsted acid
Strong acid

Products

Chemical formulaNameCoefficientTypeType in general
equation
NaClSodium chloride2
Conjugate base
Salt of strong acid
SO2Sulfur dioxide1
–
Acidic oxide
H2OWater1
Conjugate acid
Water

Thermodynamic changes

Changes in standard condition

Reaction of sodium sulfite and hydrogen chloride
◆
ΔrG−102.5 kJ/mol
K9.06 × 1017
pK−17.96
Na2SO3Crystalline solid + 2HClGas
⟶
2NaClCrystalline solid + SO2Gas + 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
−119.6−102.5−57.3737.67
per 1 mol of
−119.6−102.5−57.3737.67
per 1 mol of
−59.80−51.25−28.6818.84
per 1 mol of
−59.80−51.25−28.6818.84
per 1 mol of
−119.6−102.5−57.3737.67
per 1 mol of
−119.6−102.5−57.3737.67

Changes in aqueous solution (1)

Reaction of sodium sulfite and hydrogen chloride
◆
ΔrG−50.74 kJ/mol
K7.75 × 108
pK−8.89
Na2SO3Ionized aqueous solution + 2HClIonized aqueous solution
⟶
2NaClIonized aqueous solution + SO2Gas + 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
52.99−50.74348.2–
per 1 mol of
52.99−50.74348.2–
per 1 mol of
26.50−25.37174.1–
per 1 mol of
26.50−25.37174.1–
per 1 mol of
52.99−50.74348.2–
per 1 mol of
52.99−50.74348.2–

Changes in aqueous solution (2)

Reaction of sodium sulfite and hydrogen chloride
◆
ΔrG−51.22 kJ/mol
K9.40 × 108
pK−8.97
Na2SO3Ionized aqueous solution + 2HClIonized aqueous solution
⟶
2NaClIonized aqueous solution + SO2Un-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
26.84−51.22261.9–
per 1 mol of
26.84−51.22261.9–
per 1 mol of
13.42−25.61130.9–
per 1 mol of
13.42−25.61130.9–
per 1 mol of
26.84−51.22261.9–
per 1 mol of
26.84−51.22261.9–

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
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]–
HCl (g)-92.307[1]-95.299[1]186.908[1]29.12[1]
HCl (ai)-167.159[1]-131.228[1]56.5[1]-136.4[1]
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (g):Gas

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
NaCl (cr)-411.153[1]-384.138[1]72.13[1]50.50[1]
NaCl (g)-176.65[1]-196.66[1]229.81[1]35.77[1]
NaCl (ai)-407.27[1]-393.133[1]115.5[1]-90.0[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, (g):Gas, (ai):Ionized aqueous solution, (l):Liquid, (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)