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NiCl2 + 2NaOH → 2NaCl + Ni(OH)2

The reaction of nickel(II) chloride and sodium hydroxide yields sodium chloride and nickel(II) hydroxide (Other reactions are here). 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 reactions
  5. 5Related categories

Reaction data

Chemical equation

General equation

Oxidation state of each atom

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
NiCl2Nickel(II) chloride1
Brønsted acid
Lewis acid
Salt of weak base
Very soluble in water
NaOHSodium hydroxide2
Brønsted base
Lewis base
Strong base
Very soluble in water

Products

Chemical formulaNameCoefficientTypeType in general
equation
NaClSodium chloride2
Conjugate acid
Non-redox product
Salt of strong base
Ni(OH)2Nickel(II) hydroxide1
Conjugate base
Lewis conjugate
Weak base
Very slightly soluble in water

Thermodynamic changes

Changes in standard condition

Reaction of nickel(II) chloride and sodium hydroxide
ΔrG−197.5 kJ/mol
K3.99 × 1034
pK−34.60
NiCl2Crystalline solid + 2NaOHCrystalline solid
2NaClCrystalline solid + Ni(OH)2Crystalline solid
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
−195.5−197.56
−195.5−197.56
per 1 mol of
−97.75−98.753
per 1 mol of
−97.75−98.753
−195.5−197.56

Changes in aqueous solution

Reaction of nickel(II) chloride and sodium hydroxide
ΔrG−87.3 kJ/mol
K1.97 × 1015
pK−15.29
NiCl2Ionized aqueous solution + 2NaOHIonized aqueous solution
2NaClIonized aqueous solution + Ni(OH)2Crystalline solid
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
−15.7−87.3238
−15.7−87.3238
per 1 mol of
−7.85−43.6119
per 1 mol of
−7.85−43.6119
−15.7−87.3238

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]
NaOH (cr)-425.609[1]-379.494[1]64.455[1]59.54[1]
NaOH (g)-207.1[1]-210.0[1]228.43[1]48.37[1]
NaOH (ai)-470.114[1]-419.150[1]48.1[1]-102.1[1]
NaOH (cr)
1 hydrate
-734.543[1]-629.338[1]99.50[1]90.17[1]
NaOH (l)
2 hydrate
-1019.076[1]-873.091[1]195.979[1]239.41[1]
NaOH (l)
3.5 hydrate
-1459.798[1]-1236.356[1]286.089[1]354.43[1]
NaOH (l)
4 hydrate
-1605.15[1]-1356.64[1]318.70[1]
NaOH (l)
5 hydrate
-1894.31[1]-1596.34[1]386.06[1]
NaOH (l)
7 hydrate
-2469.02[1]-2073.80[1]526.31[1]
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (g):Gas, (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
NaCl (cr)-411.153[1]-384.138[1]72.13[1]50.50[1]
NaCl (g)-176.65[1]-196.66[1]229.81[1]35.77[1]
NaCl (ai)-407.27[1]-393.133[1]115.5[1]-90.0[1]
Ni(OH)2 (cr)-529.7[1]-447.2[1]88[1]
Ni(OH)2 (ai)-513.8[1]-360.2[1]-150.2[1]
* (cr):Crystalline solid, (g):Gas, (ai):Ionized aqueous solution

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)