You-iggy
  1. Home
  2. Chemical reactions
  3. 15KClO + 2H3AsO4 → 9KCl + 2K3AsO4 + 6ClO2↑ + 3H2O

15KClO + 2H3AsO4 → 9KCl + 2K3AsO4 + 6ClO2↑ + 3H2O

Last updated:
Reaction of potassium hypochlorite and arsenic acid
15KClOPotassium hypochlorite + 2H3AsO4Arsenic acid
⟶
9KClPotassium chloride + 2K3AsO4Potassium arsenate + 6ClO2↑Chlorine dioxide + 3H2OWater

The reaction of potassium hypochlorite and arsenic acid yields potassium chloride, potassium arsenate, chlorine dioxide, 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 + 2H3AsO4Arsenic acid
⟶
9KClPotassium chloride + 2K3AsO4Potassium arsenate + 6ClO2↑Chlorine dioxide + 3H2OWater

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 acid2
–
Acid

Products

Chemical formulaNameCoefficientTypeType in general
equation
KClPotassium chloride9
Reduced
–
K3AsO4Potassium arsenate2
–
–
ClO2Chlorine dioxide6
Oxidized
–
H2OWater3
–
–

Thermodynamic changes

Changes in aqueous solution (1)

Reaction of potassium hypochlorite and arsenic acid
◆
ΔrG−383.3 kJ/mol
K1.42 × 1067
pK−67.15
15KClOIonized aqueous solution + 2H3AsO4Un-ionized aqueous solution
⟶
9KClIonized aqueous solution + 2K3AsO4Ionized aqueous solution + 6ClO2↑Gas + 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
−112.8−383.3913–
−7.520−25.5560.9–
per 1 mol of
−56.40−191.7457–
per 1 mol of
−12.53−42.59101–
per 1 mol of
−56.40−191.7457–
per 1 mol of
−18.80−63.88152–
per 1 mol of
−37.60−127.8304–

Changes in aqueous solution (2)

Reaction of potassium hypochlorite and arsenic acid
◆
ΔrG−385.7 kJ/mol
K3.73 × 1067
pK−67.57
15KClOIonized aqueous solution + 2H3AsO4Un-ionized aqueous solution
⟶
9KClIonized aqueous solution + 2K3AsO4Ionized aqueous solution + 6ClO2↑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
−278.4−385.7361–
−18.56−25.7124.1–
per 1 mol of
−139.2−192.8181–
per 1 mol of
−30.93−42.8640.1–
per 1 mol of
−139.2−192.8181–
per 1 mol of
−46.40−64.2860.2–
per 1 mol of
−92.80−128.6120–

Changes in aqueous solution (3)

Reaction of potassium hypochlorite and arsenic acid
15KClOIonized aqueous solution + 2H3AsO4Aqueous solution
⟶
9KClIonized aqueous solution + 2K3AsO4Ionized aqueous solution + 6ClO2↑Gas + 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
−108.6–––
−7.240–––
per 1 mol of
−54.30–––
per 1 mol of
−12.07–––
per 1 mol of
−54.30–––
per 1 mol of
−18.10–––
per 1 mol of
−36.20–––

Changes in aqueous solution (4)

Reaction of potassium hypochlorite and arsenic acid
15KClOIonized aqueous solution + 2H3AsO4Aqueous solution
⟶
9KClIonized aqueous solution + 2K3AsO4Ionized aqueous solution + 6ClO2↑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
−274.2–––
−18.28–––
per 1 mol of
−137.1–––
per 1 mol of
−30.47–––
per 1 mol of
−137.1–––
per 1 mol of
−45.70–––
per 1 mol of
−91.40–––

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
KCl (cr)-436.747[1]-409.14[1]82.59[1]51.30[1]
KCl (g)-214.14[1]-233.0[1]239.10[1]36.48[1]
KCl (ai)-419.53[1]-414.49[1]159.0[1]-114.6[1]
K3AsO4 (ai)-1645.27[1]-1498.23[1]144.8[1]–
ClO2 (g)102.5[1]120.5[1]256.84[1]41.97[1]
ClO2 (ao)74.9[1]120.1[1]164.8[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]
* (cr):Crystalline solid, (g):Gas, (ai):Ionized aqueous solution, (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)