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  3. 8NaClO + 8HBrO3 → 8NaBrO3 + 2ClO2↑ + 3Cl2↑ + 4H2O

8NaClO + 8HBrO3 → 8NaBrO3 + 2ClO2↑ + 3Cl2↑ + 4H2O

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Reaction of sodium hypochlorite and bromic acid
8NaClOSodium hypochlorite + 8HBrO3Bromic acid
⟶
8NaBrO3Sodium bromate + 2ClO2↑Chlorine dioxide + 3Cl2↑Chlorine + 4H2OWater

The reaction of sodium hypochlorite and bromic acid yields sodium bromate, chlorine dioxide, 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 sodium hypochlorite and bromic acid
8NaClOSodium hypochlorite + 8HBrO3Bromic acid
⟶
8NaBrO3Sodium bromate + 2ClO2↑Chlorine dioxide + 3Cl2↑Chlorine + 4H2OWater

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 sodium hypochlorite and bromic acid

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
NaClOSodium hypochlorite8
–
Self redoxing
HBrO3Bromic acid8
–
Acid

Products

Chemical formulaNameCoefficientTypeType in general
equation
NaBrO3Sodium bromate8
–
–
ClO2Chlorine dioxide2
Oxidized
–
Cl2Chlorine3
Reduced
–
H2OWater4
–
–

Thermodynamic changes

Changes in standard condition (1)

Reaction of sodium hypochlorite and bromic acid
◆
ΔrG−413.0 kJ/mol
K2.26 × 1072
pK−72.35
8NaClOIonized aqueous solution + 8HBrO3Ionized aqueous solution
⟶
8NaBrO3Ionized aqueous solution + 2ClO2↑Gas + 3Cl2↑Gas + 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
−80.9−413.01136–
−10.1−51.63142.0–
per 1 mol of
−10.1−51.63142.0–
per 1 mol of
−10.1−51.63142.0–
per 1 mol of
−40.5−206.5568.0–
per 1 mol of
−27.0−137.7378.7–
per 1 mol of
−20.2−103.3284.0–

Changes in standard condition (2)

Reaction of sodium hypochlorite and bromic acid
◆
ΔrG−392.2 kJ/mol
K5.13 × 1068
pK−68.71
8NaClOIonized aqueous solution + 8HBrO3Ionized aqueous solution
⟶
8NaBrO3Ionized aqueous solution + 2ClO2↑Gas + 3Cl2↑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
−151.1−392.2830–
−18.89−49.02104–
per 1 mol of
−18.89−49.02104–
per 1 mol of
−18.89−49.02104–
per 1 mol of
−75.55−196.1415–
per 1 mol of
−50.37−130.7277–
per 1 mol of
−37.77−98.05208–

Changes in standard condition (3)

Reaction of sodium hypochlorite and bromic acid
◆
ΔrG−413.8 kJ/mol
K3.12 × 1072
pK−72.49
8NaClOIonized aqueous solution + 8HBrO3Ionized aqueous solution
⟶
8NaBrO3Ionized aqueous solution + 2ClO2↑Un-ionized aqueous solution + 3Cl2↑Gas + 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
−136.1−413.8952–
−17.01−51.73119–
per 1 mol of
−17.01−51.73119–
per 1 mol of
−17.01−51.73119–
per 1 mol of
−68.05−206.9476–
per 1 mol of
−45.37−137.9317–
per 1 mol of
−34.02−103.5238–

Changes in standard condition (4)

Reaction of sodium hypochlorite and bromic acid
◆
ΔrG−393.0 kJ/mol
K7.09 × 1068
pK−68.85
8NaClOIonized aqueous solution + 8HBrO3Ionized aqueous solution
⟶
8NaBrO3Ionized aqueous solution + 2ClO2↑Un-ionized aqueous solution + 3Cl2↑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
−206.3−393.0646–
−25.79−49.1380.8–
per 1 mol of
−25.79−49.1380.8–
per 1 mol of
−25.79−49.1380.8–
per 1 mol of
−103.2−196.5323–
per 1 mol of
−68.77−131.0215–
per 1 mol of
−51.58−98.25162–

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
NaClO (ai)-347.3[1]-298.7[1]100[1]–
HBrO3 (ai)-67.07[1]18.60[1]161.71[1]–
* (ai):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
NaBrO3 (cr)-334.09[1]-242.62[1]128.9[1]–
NaBrO3 (ai)-307.19[1]-243.29[1]220.9[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]–
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)