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  3. 6KI + 8NaClO2 + 8H^+ → 6KClO2 + 3I2 + Cl2↑ + 8Na^+ + 4H2O

6KI + 8NaClO2 + 8H+ → 6KClO2 + 3I2 + Cl2↑ + 8Na+ + 4H2O

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Reaction of potassium iodide and sodium chlorite under acidic condition
6KIPotassium iodide + 8NaClO2Sodium chlorite + 8H+Hydrogen ion
⟶
6KClO2Potassium chlorite + 3I2Iodine + Cl2↑Chlorine + 8Na+Sodium ion + 4H2OWater

The reaction of potassium iodide, sodium chlorite, and hydrogen ion yields potassium chlorite, iodine, chlorine, sodium 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 potassium iodide and sodium chlorite under acidic condition
6KIPotassium iodide + 8NaClO2Sodium chlorite + 8H+Hydrogen ion
⟶
6KClO2Potassium chlorite + 3I2Iodine + Cl2↑Chlorine + 8Na+Sodium ion + 4H2OWater

General equation

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

Oxidation state of each atom

Reaction of potassium iodide and sodium chlorite under acidic condition

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
KIPotassium iodide6
Reducing
Oxidizable
NaClO2Sodium chlorite8
Oxidizing
Oxidizing under acidic condition
H+Hydrogen ion8
–
Hydrogen ion

Products

Chemical formulaNameCoefficientTypeType in general
equation
KClO2Potassium chlorite6
–
–
I2Iodine3
Oxidized
–
Cl2Chlorine1
Reduced
–
Na+Sodium ion8
–
–
H2OWater4
–
Water

Thermodynamic changes

Changes in aqueous solution (1)

Reaction of potassium iodide and sodium chlorite under acidic condition
◆
ΔrG−624.5 kJ/mol
K2.56 × 10109
pK−109.41
6KIIonized aqueous solution + 8NaClO2Ionized aqueous solution + 8H+Un-ionized aqueous solution
⟶
6KClO2Ionized aqueous solution + 3I2Un-ionized aqueous solution + Cl2↑Gas + 8Na+Un-ionized aqueous solution + 4H2OLiquid
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
−610.3−624.544.7–
per 1 mol of
−101.7−104.17.45–
per 1 mol of
−76.29−78.065.59–
per 1 mol of
Hydrogen ion
−76.29−78.065.59–
per 1 mol of
−101.7−104.17.45–
per 1 mol of
−203.4−208.214.9–
per 1 mol of
−610.3−624.544.7–
per 1 mol of
Sodium ion
−76.29−78.065.59–
per 1 mol of
−152.6−156.111.2–

Changes in aqueous solution (2)

Reaction of potassium iodide and sodium chlorite under acidic condition
◆
ΔrG−617.5 kJ/mol
K1.52 × 10108
pK−108.18
6KIIonized aqueous solution + 8NaClO2Ionized aqueous solution + 8H+Un-ionized aqueous solution
⟶
6KClO2Ionized aqueous solution + 3I2Un-ionized aqueous solution + Cl2↑Un-ionized aqueous solution + 8Na+Un-ionized aqueous solution + 4H2OLiquid
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
−633.7−617.5−57–
per 1 mol of
−105.6−102.9−9.5–
per 1 mol of
−79.21−77.19−7.1–
per 1 mol of
Hydrogen ion
−79.21−77.19−7.1–
per 1 mol of
−105.6−102.9−9.5–
per 1 mol of
−211.2−205.8−19–
per 1 mol of
−633.7−617.5−57–
per 1 mol of
Sodium ion
−79.21−77.19−7.1–
per 1 mol of
−158.4−154.4−14–

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
KI (cr)-327.900[1]-324.892[1]106.32[1]52.93[1]
KI (g)-125.5[1]-166.1[1]258.3[1]37.11[1]
KI (ai)-307.57[1]-334.85[1]213.8[1]-120.5[1]
NaClO2 (cr)-307.02[1]–––
NaClO2 (ai)-306.7[1]-244.7[1]160.2[1]–
NaClO2 (cr)
3 hydrate
-1192.77[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
KClO2 (ai)-318.8[1]-266.1[1]203.8[1]–
I2 (cr)0[1]0[1]116.135[1]54.438[1]
I2 (g)62.438[1]19.327[1]260.69[1]36.90[1]
I2 (ao)22.6[1]16.40[1]137.2[1]–
Cl2 (g)0[1]0[1]223.066[1]33.907[1]
Cl2 (ao)-23.4[1]6.94[1]121[1]–
Na+ (g)609.358[1]–––
Na+ (ao)-240.12[1]-261.905[1]59.0[1]46.4[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]
* (ai):Ionized aqueous solution, (cr):Crystalline solid, (g):Gas, (ao):Un-ionized aqueous solution, (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)