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3NaClO + 2HBrO3 → NaClO3 + 2NaBrO3 + 2HCl↑

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Reaction of sodium hypochlorite and bromic acid
3NaClOSodium hypochlorite + 2HBrO3Bromic acid
⟶
NaClO3Sodium chlorate + 2NaBrO3Sodium bromate + 2HCl↑Hydrogen chloride

The reaction of sodium hypochlorite and bromic acid yields sodium chlorate, sodium bromate, and hydrogen chloride (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
3NaClOSodium hypochlorite + 2HBrO3Bromic acid
⟶
NaClO3Sodium chlorate + 2NaBrO3Sodium bromate + 2HCl↑Hydrogen chloride

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 hypochlorite3
–
Self redoxing
HBrO3Bromic acid2
–
Acid

Products

Chemical formulaNameCoefficientTypeType in general
equation
NaClO3Sodium chlorate1
Oxidized
–
NaBrO3Sodium bromate2
–
–
HClHydrogen chloride2
Reduced
–

Thermodynamic changes

Changes in standard condition (1)

Reaction of sodium hypochlorite and bromic acid
◆
ΔrG−88.1 kJ/mol
K2.72 × 1015
pK−15.43
3NaClOIonized aqueous solution + 2HBrO3Ionized aqueous solution
⟶
NaClO3Ionized aqueous solution + 2NaBrO3Ionized aqueous solution + 2HCl↑Gas
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
33.0−88.1413–
11.0−29.4138–
per 1 mol of
16.5−44.0207–
per 1 mol of
33.0−88.1413–
per 1 mol of
16.5−44.0207–
per 1 mol of
16.5−44.0207–

Changes in standard condition (2)

Reaction of sodium hypochlorite and bromic acid
◆
ΔrG−160.0 kJ/mol
K1.07 × 1028
pK−28.03
3NaClOIonized aqueous solution + 2HBrO3Ionized aqueous solution
⟶
NaClO3Ionized aqueous solution + 2NaBrO3Ionized aqueous solution + 2HCl↑Ionized aqueous solution
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
−116.7−160.0153–
−38.90−53.3351.0–
per 1 mol of
−58.35−80.0076.5–
per 1 mol of
−116.7−160.0153–
per 1 mol of
−58.35−80.0076.5–
per 1 mol of
−58.35−80.0076.5–

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
NaClO3 (cr)-365.774[1]-262.259[1]123.4[1]–
NaClO3 (ai)-344.09[1]-269.84[1]221.3[1]–
NaBrO3 (cr)-334.09[1]-242.62[1]128.9[1]–
NaBrO3 (ai)-307.19[1]-243.29[1]220.9[1]–
HCl (g)-92.307[1]-95.299[1]186.908[1]29.12[1]
HCl (ai)-167.159[1]-131.228[1]56.5[1]-136.4[1]
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (g):Gas

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)