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MnSiO3 + 2NaOH → Na2SiO3 + Mn(OH)2

The reaction of manganese(II) metasilicate and sodium hydroxide yields sodium metasilicate and manganese(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
MnSiO3Manganese(II) metasilicate1
Brønsted acid
Salt of weak base
NaOHSodium hydroxide2
Brønsted base
Strong base

Products

Chemical formulaNameCoefficientTypeType in general
equation
Na2SiO3Sodium metasilicate1
Conjugate acid
Salt of strong base
Mn(OH)2Manganese(II) hydroxide1
Conjugate base
Weak base

Thermodynamic changes

Changes in standard condition

Reaction of manganese(II) metasilicate and sodium hydroxide
ΔrG−78.3 kJ/mol
K5.22 × 1013
pK−13.72
MnSiO3Crystalline solid + 2NaOHCrystalline solid
Na2SiO3Crystalline solid + Mn(OH)2Amorphous 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
−78.2−78.3−5.0
−78.2−78.3−5.0
per 1 mol of
−39.1−39.1−2.5
−78.2−78.3−5.0
−78.2−78.3−5.0

Changes in aqueous solution

Reaction of manganese(II) metasilicate and sodium hydroxide
MnSiO3Crystalline solid + 2NaOHIonized aqueous solution
Na2SiO3Aqueous solution + Mn(OH)2Amorphous 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
−20.5
−20.5
per 1 mol of
−10.3
−20.5
−20.5

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
MnSiO3 (cr)-1320.9[1]-1240.5[1]89.1[1]86.44[1]
MnSiO3 (vit)-1285.3[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, (vit):Vitreous liquid, (g):Gas, (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
Na2SiO3 (cr)-1554.90[1]-1462.80[1]113.85[1]
Na2SiO3 (vit)-1540.1[1]
Na2SiO3 (aq)-1586.2[1]
Na2SiO3 (cr)
5 hydrate
-3048.5[1]
Na2SiO3 (cr)
9 hydrate
-4228.8[1]
Mn(OH)2 (am)
precipitated
-695.4[1]-615.0[1]99.2[1]
* (cr):Crystalline solid, (vit):Vitreous liquid, (aq):Aqueous solution, (am):Amorphous solid

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)