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  3. 8NaHSO4 + 8e^− → 7NaSO4^− + Na^+ + S^2− + 4H2O

8NaHSO4 + 8e− → 7NaSO4− + Na+ + S2− + 4H2O

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Reduction of sodium hydrogensulfate
8NaHSO4Sodium hydrogensulfate + 8e−Electron
⟶
7NaSO4−Sodium sulfate ion + Na+Sodium ion + S2−Sulfide ion + 4H2OWater

Reduction of sodium hydrogensulfate yields sodium sulfate ion, sodium ion, sulfide ion, 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

Reduction of sodium hydrogensulfate
8NaHSO4Sodium hydrogensulfate + 8e−Electron
⟶
7NaSO4−Sodium sulfate ion + Na+Sodium ion + S2−Sulfide ion + 4H2OWater

General equation

Reduction of reducible species
ReactantOxidizing agent + e−
⟶
ProductReduction product

Oxidation state of each atom

Reduction of sodium hydrogensulfate

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
NaHSO4Sodium hydrogensulfate8
Oxidizing
–
e−Electron8
–
Electron

Products

Chemical formulaNameCoefficientTypeType in general
equation
NaSO4−Sodium sulfate ion7
–
–
Na+Sodium ion1
–
–
S2−Sulfide ion1
Reduced
–
H2OWater4
–
–

Thermodynamic changes

Changes in standard condition

Reduction of sodium hydrogensulfate
◆
ΔrG−56.5 kJ/mol
K7.91 × 109
pK−9.90
8NaHSO4Ionized aqueous solution + 8e−
⟶
7NaSO4−Un-ionized aqueous solution + Na+Un-ionized aqueous solution + S2−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
−343.6−56.5−440.8–
−42.95−7.06−55.10–
per 1 mol of
Electron
−42.95−7.06−55.10–
per 1 mol of
Sodium sulfate ion
−49.09−8.07−62.97–
per 1 mol of
Sodium ion
−343.6−56.5−440.8–
per 1 mol of
Sulfide ion
−343.6−56.5−440.8–
per 1 mol of
−85.90−14.1−110.2–

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
NaHSO4 (cr)-1125.5[1]-992.8[1]113.0[1]–
NaHSO4 (ai)-1127.46[1]-1017.80[1]190.8[1]-38[1]
NaHSO4 (cr)
1 hydrate
-1421.7[1]-1231.6[1]155[1]–
e−––––
* (cr):Crystalline solid, (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
NaSO4− (ao)-1144.70[1]-1010.61[1]108.8[1]–
Na+ (g)609.358[1]–––
Na+ (ao)-240.12[1]-261.905[1]59.0[1]46.4[1]
S2− (ao)33.1[1]85.8[1]-14.6[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]
* (ao):Un-ionized aqueous solution, (g):Gas, (cr):Crystalline solid, (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)