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  3. 3NaCl + 5KClO + 8H^+ → 3Na^+ + 2HClO + 3Cl2↑ + 5K^+ + 3H2O

3NaCl + 5KClO + 8H+ → 3Na+ + 2HClO + 3Cl2↑ + 5K+ + 3H2O

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Reaction of sodium chloride and potassium hypochlorite under acidic condition
3NaClSodium chloride + 5KClOPotassium hypochlorite + 8H+Hydrogen ion
⟶
3Na+Sodium ion + 2HClOHypochlorous acid + 3Cl2↑Chlorine + 5K+Potassium ion + 3H2OWater

The reaction of sodium chloride, potassium hypochlorite, and hydrogen ion yields sodium ion, hypochlorous acid, chlorine, potassium ion, and water (Other reactions are here). This reaction is an oxidation-reduction 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 chloride and potassium hypochlorite under acidic condition
3NaClSodium chloride + 5KClOPotassium hypochlorite + 8H+Hydrogen ion
⟶
3Na+Sodium ion + 2HClOHypochlorous acid + 3Cl2↑Chlorine + 5K+Potassium ion + 3H2OWater

General equation

Reaction of hardly oxidizable species and oxidizing species under acidic condition
Hardly oxidizable speciesReducing agent + Oxidizing speciesOxidizing agent + H+Non-redox agent
⟶
ProductOxidation product + ProductReduction product + H2ONon-redox product

Oxidation state of each atom

Reaction of sodium chloride and potassium hypochlorite under acidic condition

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
NaClSodium chloride3
Reducing
Hardly oxidizable
KClOPotassium hypochlorite5
Oxidizing
Oxidizing under acidic condition
H+Hydrogen ion8
–
Hydrogen ion

Products

Chemical formulaNameCoefficientTypeType in general
equation
Na+Sodium ion3
–
–
HClOHypochlorous acid2
–
–
Cl2Chlorine3
Redoxed product
–
K+Potassium ion5
–
–
H2OWater3
–
Water

Thermodynamic changes

Changes in aqueous solution (1)

Reaction of sodium chloride and potassium hypochlorite under acidic condition
◆
ΔrG−293.9 kJ/mol
K3.08 × 1051
pK−51.49
3NaClIonized aqueous solution + 5KClOIonized aqueous solution + 8H+Un-ionized aqueous solution
⟶
3Na+Un-ionized aqueous solution + 2HClOUn-ionized aqueous solution + 3Cl2↑Gas + 5K+Un-ionized aqueous solution + 3H2OLiquid
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
−62.7−293.9776–
per 1 mol of
−20.9−97.97259–
−12.5−58.78155–
per 1 mol of
Hydrogen ion
−7.84−36.7497.0–
per 1 mol of
Sodium ion
−20.9−97.97259–
per 1 mol of
−31.4−146.9388–
per 1 mol of
−20.9−97.97259–
per 1 mol of
Potassium ion
−12.5−58.78155–
per 1 mol of
−20.9−97.97259–

Changes in aqueous solution (2)

Reaction of sodium chloride and potassium hypochlorite under acidic condition
◆
ΔrG−273.0 kJ/mol
K6.72 × 1047
pK−47.83
3NaClIonized aqueous solution + 5KClOIonized aqueous solution + 8H+Un-ionized aqueous solution
⟶
3Na+Un-ionized aqueous solution + 2HClOUn-ionized aqueous solution + 3Cl2↑Un-ionized aqueous solution + 5K+Un-ionized aqueous solution + 3H2OLiquid
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
−132.9−273.0470–
per 1 mol of
−44.30−91.00157–
−26.58−54.6094.0–
per 1 mol of
Hydrogen ion
−16.61−34.1358.8–
per 1 mol of
Sodium ion
−44.30−91.00157–
per 1 mol of
−66.45−136.5235–
per 1 mol of
−44.30−91.00157–
per 1 mol of
Potassium ion
−26.58−54.6094.0–
per 1 mol of
−44.30−91.00157–

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
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]
KClO (ai)-359.4[1]-320.0[1]146[1]–
H+ (g)1536.202[1]–––
H+ (ao)0[1]0[1]0[1]0[1]
* (cr):Crystalline solid, (g):Gas, (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
Na+ (g)609.358[1]–––
Na+ (ao)-240.12[1]-261.905[1]59.0[1]46.4[1]
HClO (g)-78.7[1]-66.1[1]236.67[1]37.15[1]
HClO (ao)-120.9[1]-79.9[1]142[1]–
Cl2 (g)0[1]0[1]223.066[1]33.907[1]
Cl2 (ao)-23.4[1]6.94[1]121[1]–
K+ (g)514.26[1]–––
K+ (ao)-252.38[1]-283.27[1]102.5[1]21.8[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]
* (g):Gas, (ao):Un-ionized aqueous solution, (cr):Crystalline solid, (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)