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NiCl2 + H2SO4 → NiSO4 + 2HCl↑

The reaction of nickel(II) chloride and sulfuric acid yields nickel(II) sulfate and hydrogen chloride. This reaction is an acid-base reaction and is classified as follows:

Table of contents
  1. 1Reaction data
  2. 2Thermodynamic changes
  3. 3References
  4. 4Related categories

Reaction data

Chemical equation

General equation

Oxidation state of each atom

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
NiCl2Nickel(II) chloride1
Brønsted base
Salt of volatile acid
H2SO4Sulfuric acid1
Brønsted acid
Nonvolatile acid

Products

Chemical formulaNameCoefficientTypeType in general
equation
NiSO4Nickel(II) sulfate1
Conjugate base
Salt of non volatile acid
HClHydrogen chloride2
Conjugate acid
Volatile acid

Thermodynamic changes

Changes in standard condition

Reaction of nickel(II) chloride and sulfuric acid
ΔrG−1.3 kJ/mol
K1.69 × 100
pK−0.23
NiCl2Crystalline solid + H2SO4Liquid
NiSO4Crystalline solid + 2HClGas
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
61.80−1.3211−14
61.80−1.3211−14
per 1 mol of
61.80−1.3211−14
per 1 mol of
61.80−1.3211−14
per 1 mol of
30.90−0.65106−7.0

Changes in aqueous solution (1)

Reaction of nickel(II) chloride and sulfuric acid
ΔrG71.5 kJ/mol
K0.30 × 10−12
pK12.53
NiCl2Ionized aqueous solution + H2SO4Ionized aqueous solution
NiSO4Ionized aqueous solution + 2HClGas
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
149.871.5260.0
149.871.5260.0
per 1 mol of
149.871.5260.0
per 1 mol of
149.871.5260.0
per 1 mol of
74.9035.8130.0

Changes in aqueous solution (2)

Reaction of nickel(II) chloride and sulfuric acid
ΔrG−0.3 kJ/mol
K1.13 × 100
pK−0.05
NiCl2Ionized aqueous solution + H2SO4Ionized aqueous solution
NiSO4Ionized aqueous solution + 2HClIonized 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
0.1−0.3−0.8
0.10−0.30−0.80
per 1 mol of
0.10−0.30−0.80
per 1 mol of
0.10−0.30−0.80
per 1 mol of
0.050−0.15−0.40

Changes in aqueous solution (3)

Reaction of nickel(II) chloride and sulfuric acid
ΔrG58.5 kJ/mol
K0.56 × 10−10
pK10.25
NiCl2Ionized aqueous solution + H2SO4Ionized aqueous solution
NiSO4Un-ionized aqueous solution + 2HClGas
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
163.758.5350.8
163.758.5350.8
per 1 mol of
163.758.5350.8
per 1 mol of
163.758.5350.8
per 1 mol of
81.8529.3175.4

Changes in aqueous solution (4)

Reaction of nickel(II) chloride and sulfuric acid
ΔrG−13.3 kJ/mol
K2.14 × 102
pK−2.33
NiCl2Ionized aqueous solution + H2SO4Ionized aqueous solution
NiSO4Un-ionized aqueous solution + 2HClIonized 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
14.0−13.390.0
14.0−13.390.0
per 1 mol of
14.0−13.390.0
per 1 mol of
14.0−13.390.0
per 1 mol of
7.00−6.6545.0

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
NiCl2 (cr)-305.332[1]-259.032[1]97.65[1]71.67[1]
NiCl2 (ai)-388.3[1]-307.9[1]-15.1[1]
NiCl2 (cr)
2 hydrate
-922.2[1]-760.1[1]176[1]
NiCl2 (cr)
4 hydrate
-1516.7[1]-1234.9[1]243[1]
NiCl2 (cr)
6 hydrate
-2103.17[1]-1713.19[1]344.3[1]
H2SO4 (cr)
H2SO4 (l)-813.989[1]-690.003[1]156.904[1]138.91[1]
H2SO4 (ai)-909.27[1]-744.53[1]20.1[1]-293[1]
H2SO4 (l)
1 hydrate
-1127.621[1]-950.383[1]211.54[1]214.85[1]
H2SO4 (l)
2 hydrate
-1427.100[1]-1199.650[1]276.40[1]260.83[1]
H2SO4 (l)
3 hydrate
-1720.402[1]-1443.980[1]345.39[1]318.95[1]
H2SO4 (l)
4 hydrate
-2011.199[1]-1685.863[1]414.59[1]382.21[1]
H2SO4 (l)
6.5 hydrate
-2733.256[1]-2285.734[1]587.89[1]570.28[1]
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (l):Liquid

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
NiSO4 (cr)-872.91[1]-759.7[1]92[1]138[1]
NiSO4 (ai)-963.2[1]-790.3[1]-108.8[1]
NiSO4 (ao)-949.3[1]-803.3[1]-18.0[1]
NiSO4 (cr)
4 hydrate
-2104.1[1]
NiSO4 (cr)
6 hydrate
α, tetragonal, green
-2682.82[1]-2224.61[1]334.47[1]327.86[1]
NiSO4 (cr)
6 hydrate
β, monoclinic, blue
-2672.3[1]
NiSO4 (cr)
7 hydrate
-2976.33[1]-2461.83[1]378.94[1]364.59[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, (ao):Un-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)