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PbCl2 + 2NaOH → 2NaCl + Pb(OH)2

The reaction of lead(II) chloride and sodium hydroxide yields sodium chloride and lead(II) hydroxide. 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
PbCl2Lead(II) chloride1
Brønsted acid
Salt of weak base
NaOHSodium hydroxide2
Brønsted base
Strong base

Products

Chemical formulaNameCoefficientTypeType in general
equation
NaClSodium chloride2
Conjugate acid
Salt of strong base
Pb(OH)2Lead(II) hydroxide1
Conjugate base
Weak base

Thermodynamic changes

Changes in standard condition (1)

Reaction of lead(II) chloride and sodium hydroxide
ΔrG−147.4 kJ/mol
K6.66 × 1025
pK−25.82
PbCl2Crystalline solid + 2NaOHCrystalline solid
2NaClCrystalline solid + Pb(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
−147.4
per 1 mol of
−147.4
per 1 mol of
−73.70
per 1 mol of
−73.70
per 1 mol of
−147.4

Changes in standard condition (2)

Reaction of lead(II) chloride and sodium hydroxide
PbCl2Crystalline solid + 2NaOHCrystalline solid
2NaClCrystalline solid + Pb(OH)2Crystalline solidprecipitated
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
−127.6
per 1 mol of
−127.6
per 1 mol of
−63.80
per 1 mol of
−63.80
per 1 mol of
−127.6

Changes in aqueous solution (1)

Reaction of lead(II) chloride and sodium hydroxide
ΔrG−113.3 kJ/mol
K7.07 × 1019
pK−19.85
PbCl2Ionized aqueous solution + 2NaOHIonized aqueous solution
2NaClIonized aqueous solution + Pb(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
−113.3
per 1 mol of
−113.3
per 1 mol of
−56.65
per 1 mol of
−56.65
per 1 mol of
−113.3

Changes in aqueous solution (2)

Reaction of lead(II) chloride and sodium hydroxide
ΔrG−103.0 kJ/mol
K1.11 × 1018
pK−18.04
PbCl2Un-ionized aqueous solution + 2NaOHIonized aqueous solution
2NaClIonized aqueous solution + Pb(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
−103.0
per 1 mol of
−103.0
per 1 mol of
−51.50
per 1 mol of
−51.50
per 1 mol of
−103.0

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
PbCl2 (cr)-359.41[1]-314.10[1]136.0[1]
PbCl2 (ai)-336.0[1]-286.86[1]123.4[1]
PbCl2 (ao)-297.16[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, (ao):Un-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]
Pb(OH)2 (cr)-452.2[1]
Pb(OH)2 (cr)
precipitated
-515.9[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)