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15KClO + 4H3AsO4 → 3KClO3 + 4K3AsO4 + 6Cl2↑ + 6H2O

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Reaction of potassium hypochlorite and arsenic acid
15KClOPotassium hypochlorite + 4H3AsO4Arsenic acid
⟶
3KClO3Potassium chlorate + 4K3AsO4Potassium arsenate + 6Cl2↑Chlorine + 6H2OWater

The reaction of potassium hypochlorite and arsenic acid yields potassium chlorate, potassium arsenate, chlorine, 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 hypochlorite and arsenic acid
15KClOPotassium hypochlorite + 4H3AsO4Arsenic acid
⟶
3KClO3Potassium chlorate + 4K3AsO4Potassium arsenate + 6Cl2↑Chlorine + 6H2OWater

General equation

Reaction of self redoxing species and acid
Self-redoxing speciesSelf redox agent + AcidNon-redox agent
⟶
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Reaction of potassium hypochlorite and arsenic acid

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
KClOPotassium hypochlorite15
–
Self redoxing
H3AsO4Arsenic acid4
–
Acid

Products

Chemical formulaNameCoefficientTypeType in general
equation
KClO3Potassium chlorate3
Oxidized
–
K3AsO4Potassium arsenate4
–
–
Cl2Chlorine6
Reduced
–
H2OWater6
–
–

Thermodynamic changes

Changes in aqueous solution (1)

Reaction of potassium hypochlorite and arsenic acid
◆
ΔrG−425.4 kJ/mol
K3.36 × 1074
pK−74.53
15KClOIonized aqueous solution + 4H3AsO4Un-ionized aqueous solution
⟶
3KClO3Ionized aqueous solution + 4K3AsO4Ionized aqueous solution + 6Cl2↑Gas + 6H2OLiquid
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
−364.1−425.4205–
−24.27−28.3613.7–
per 1 mol of
−91.03−106.351.3–
per 1 mol of
−121.4−141.868.3–
per 1 mol of
−91.03−106.351.3–
per 1 mol of
−60.68−70.9034.2–
per 1 mol of
−60.68−70.9034.2–

Changes in aqueous solution (2)

Reaction of potassium hypochlorite and arsenic acid
◆
ΔrG−383.7 kJ/mol
K1.66 × 1067
pK−67.22
15KClOIonized aqueous solution + 4H3AsO4Un-ionized aqueous solution
⟶
3KClO3Ionized aqueous solution + 4K3AsO4Ionized aqueous solution + 6Cl2↑Un-ionized aqueous solution + 6H2OLiquid
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
−504.5−383.7−407–
−33.63−25.58−27.1–
per 1 mol of
−126.1−95.92−102–
per 1 mol of
−168.2−127.9−136–
per 1 mol of
−126.1−95.92−102–
per 1 mol of
−84.08−63.95−67.8–
per 1 mol of
−84.08−63.95−67.8–

Changes in aqueous solution (3)

Reaction of potassium hypochlorite and arsenic acid
15KClOIonized aqueous solution + 4H3AsO4Aqueous solution
⟶
3KClO3Ionized aqueous solution + 4K3AsO4Ionized aqueous solution + 6Cl2↑Gas + 6H2OLiquid
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
−355.7–––
−23.71–––
per 1 mol of
−88.92–––
per 1 mol of
−118.6–––
per 1 mol of
−88.92–––
per 1 mol of
−59.28–––
per 1 mol of
−59.28–––

Changes in aqueous solution (4)

Reaction of potassium hypochlorite and arsenic acid
15KClOIonized aqueous solution + 4H3AsO4Aqueous solution
⟶
3KClO3Ionized aqueous solution + 4K3AsO4Ionized aqueous solution + 6Cl2↑Un-ionized aqueous solution + 6H2OLiquid
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
−496.1–––
−33.07–––
per 1 mol of
−124.0–––
per 1 mol of
−165.4–––
per 1 mol of
−124.0–––
per 1 mol of
−82.68–––
per 1 mol of
−82.68–––

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
KClO (ai)-359.4[1]-320.0[1]146[1]–
H3AsO4 (cr)-906.3[1]–––
H3AsO4 (ao)-902.5[1]-766.0[1]184[1]–
H3AsO4 (aq)-904.6[1]–––
* (ai):Ionized aqueous solution, (cr):Crystalline solid, (ao):Un-ionized aqueous solution, (aq):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
KClO3 (cr)-397.73[1]-296.25[1]143.1[1]100.25[1]
KClO3 (ai)-356.35[1]-291.22[1]264.8[1]–
K3AsO4 (ai)-1645.27[1]-1498.23[1]144.8[1]–
Cl2 (g)0[1]0[1]223.066[1]33.907[1]
Cl2 (ao)-23.4[1]6.94[1]121[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, (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)