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3NaClO + 4H3BO3 ๐Ÿ”ฅโ†’ NaClO2 + Na2B4O7 + Cl2โ†‘ + 6H2O

The reaction of sodium hypochlorite and boric acid yields sodium chlorite, sodium tetraborate, 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

General equation

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

Oxidation state of each atom

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
NaClOSodium hypochlorite3
โ€“
Self redoxing
H3BO3Boric acid4
โ€“
Acid

Products

Chemical formulaNameCoefficientTypeType in general
equation
NaClO2Sodium chlorite1
Oxidized
โ€“
Na2B4O7Sodium tetraborate1
โ€“
โ€“
Cl2Chlorine1
Reduced
โ€“
H2OWater6
โ€“
โ€“

Thermodynamic changes

Changes in aqueous solution (1)

Reaction of sodium hypochlorite and boric acid
โ—†
ฮ”rGโˆ’25.1 kJ/mol
K2.50 ร— 104
pKโˆ’4.40
3NaClOIonized aqueous solution + 4H3BO3Un-ionized aqueous solution
๐Ÿ”ฅ
โŸถ
NaClO2Ionized aqueous solution + Na2B4O7Ionized aqueous solution + Cl2โ†‘Gas + 6H2OLiquid
Standard enthalpy
of reaction
ฮ”rHยฐ
kJ ยท molโˆ’1
Standard
Gibbs energy
of reaction
ฮ”rGยฐ
kJ ยท molโˆ’1
Standard entropy
of reaction
ฮ”rSยฐ
J ยท Kโˆ’1 ยท molโˆ’1
Standard heat
capacity of reaction
at constant pressure
ฮ”rCpยฐ
J ยท Kโˆ’1 ยท molโˆ’1
per 1 mol of
Equation
โ€“โˆ’25.1โ€“โ€“
โ€“โˆ’8.37โ€“โ€“
per 1 mol of
โ€“โˆ’6.28โ€“โ€“
per 1 mol of
โ€“โˆ’25.1โ€“โ€“
per 1 mol of
โ€“โˆ’25.1โ€“โ€“
per 1 mol of
โ€“โˆ’25.1โ€“โ€“
per 1 mol of
โ€“โˆ’4.18โ€“โ€“

Changes in aqueous solution (2)

Reaction of sodium hypochlorite and boric acid
โ—†
ฮ”rGโˆ’18.1 kJ/mol
K1.48 ร— 103
pKโˆ’3.17
3NaClOIonized aqueous solution + 4H3BO3Un-ionized aqueous solution
๐Ÿ”ฅ
โŸถ
NaClO2Ionized aqueous solution + Na2B4O7Ionized aqueous solution + Cl2โ†‘Un-ionized aqueous solution + 6H2OLiquid
Standard enthalpy
of reaction
ฮ”rHยฐ
kJ ยท molโˆ’1
Standard
Gibbs energy
of reaction
ฮ”rGยฐ
kJ ยท molโˆ’1
Standard entropy
of reaction
ฮ”rSยฐ
J ยท Kโˆ’1 ยท molโˆ’1
Standard heat
capacity of reaction
at constant pressure
ฮ”rCpยฐ
J ยท Kโˆ’1 ยท molโˆ’1
per 1 mol of
Equation
โ€“โˆ’18.1โ€“โ€“
โ€“โˆ’6.03โ€“โ€“
per 1 mol of
โ€“โˆ’4.53โ€“โ€“
per 1 mol of
โ€“โˆ’18.1โ€“โ€“
per 1 mol of
โ€“โˆ’18.1โ€“โ€“
per 1 mol of
โ€“โˆ’18.1โ€“โ€“
per 1 mol of
โ€“โˆ’3.02โ€“โ€“

Thermodynamic data of reactants

Chemical formulaStandard enthalpy
of formation
ฮ”fHยฐ
kJ ยท molโˆ’1
Standard Gibbs
energy of
formation
ฮ”fGยฐ
kJ ยท molโˆ’1
Standard
molar entropy
Sยฐ
J ยท Kโˆ’1 ยท molโˆ’1
Standard molar
heat capacity at
constant pressure
Cpยฐ
J ยท Kโˆ’1 ยท molโˆ’1
NaClO (ai)-347.3[1]-298.7[1]100[1]โ€“
H3BO3 (cr)-1094.33[1]-968.92[1]88.83[1]81.38[1]
H3BO3 (g)-994.1[1]โ€“โ€“โ€“
H3BO3 (ao)-1072.32[1]-968.75[1]162.3[1]โ€“
* (ai):Ionized aqueous solution, (cr):Crystalline solid, (g):Gas, (ao):Un-ionized aqueous solution

Thermodynamic data of products

Chemical formulaStandard enthalpy
of formation
ฮ”fHยฐ
kJ ยท molโˆ’1
Standard Gibbs
energy of
formation
ฮ”fGยฐ
kJ ยท molโˆ’1
Standard
molar entropy
Sยฐ
J ยท Kโˆ’1 ยท molโˆ’1
Standard molar
heat capacity at
constant pressure
Cpยฐ
J ยท Kโˆ’1 ยท molโˆ’1
NaClO2 (cr)-307.02[1]โ€“โ€“โ€“
NaClO2 (ai)-306.7[1]-244.7[1]160.2[1]โ€“
NaClO2 (cr)
3 hydrate
-1192.77[1]โ€“โ€“โ€“
Na2B4O7 (cr)-3291.1[1]-3096.0[1]189.54[1]186.77[1]
Na2B4O7 (am)-3271.1[1]-3076.8[1]192.9[1]โ€“
Na2B4O7 (ai)โ€“-3128.7[1]โ€“โ€“
Na2B4O7 (cr)
4 hydrate
-4507.4[1]โ€“โ€“โ€“
Na2B4O7 (cr)
5 hydrate
-4802.4[1]โ€“โ€“โ€“
Na2B4O7 (cr)
10 hydrate
-6288.6[1]-5516.0[1]586[1]615[1]
Cl2 (g)0[1]0[1]223.066[1]33.907[1]
Cl2 (ao)-23.4[1]6.94[1]121[1]โ€“
H2O (cr)โ€“โ€“โ€“โ€“
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, (am):Amorphous 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)