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CoSO4 + Mg(OH)2 → MgSO4 + Co(OH)2

CoSO₄ + Mg(OH)₂ → MgSO₄ + Co(OH)₂

Last updated: June 13, 2022

Reaction of cobalt(II) sulfate and magnesium hydroxide: CoSO₄Cobalt(II) sulfate + Mg(OH)₂Magnesium hydroxide
⟶
MgSO₄Magnesium sulfate + Co(OH)₂Cobalt(II) hydroxide

The reaction of cobalt(II) sulfate and magnesium hydroxide yields magnesium sulfate and cobalt(II) hydroxide. This reaction is an acid-base reaction and is classified as follows:

Reaction of salt of weak base and strong base

Table of contents

Reaction data

Reactants

Chemical formula	Name	Coefficient	Type	Type in general equation
CoSO₄	Cobalt(II) sulfate	1	Brønsted acid	Salt of weak base
Mg(OH)₂	Magnesium hydroxide	1	Brønsted base	Strong base

Products

Chemical formula	Name	Coefficient	Type	Type in general equation
MgSO₄	Magnesium sulfate	1	Conjugate acid	Salt of strong base
Co(OH)₂	Cobalt(II) hydroxide	1	Conjugate base	Weak base

Thermodynamic changes

Changes in standard condition (1)

Reaction of cobalt(II) sulfate and magnesium hydroxide ◆ Δ_rG −4.9 kJ/mol K 7.22 × 10⁰ pK −0.86: CoSO₄Crystalline solid + Mg(OH)₂Crystalline solid
⟶
MgSO₄Crystalline solid + Co(OH)₂Crystalline solidblue, precipitated

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard entropy of reaction Δ_rS° J · K⁻¹ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	–	−4.9	–	–
per 1 mol of Cobalt(II) sulfate	–	−4.9	–	–
per 1 mol of Magnesium hydroxide	–	−4.9	–	–
per 1 mol of Magnesium sulfate	–	−4.9	–	–
per 1 mol of Cobalt(II) hydroxide	–	−4.9	–	–

Changes in standard condition (2)

Reaction of cobalt(II) sulfate and magnesium hydroxide ◆ Δ_rG −9.1 kJ/mol K 3.93 × 10¹ pK −1.59: CoSO₄Crystalline solid + Mg(OH)₂Crystalline solid
⟶
MgSO₄Crystalline solid + Co(OH)₂Crystalline solidpink, precipitated

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard entropy of reaction Δ_rS° J · K⁻¹ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	−11.8	−9.1	−11	–
per 1 mol of Cobalt(II) sulfate	−11.8	−9.1	−11	–
per 1 mol of Magnesium hydroxide	−11.8	−9.1	−11	–
per 1 mol of Magnesium sulfate	−11.8	−9.1	−11	–
per 1 mol of Cobalt(II) hydroxide	−11.8	−9.1	−11	–

Changes in standard condition (3)

Reaction of cobalt(II) sulfate and magnesium hydroxide ◆ Δ_rG −12.9 kJ/mol K 1.82 × 10² pK −2.26: CoSO₄Crystalline solid + Mg(OH)₂Crystalline solid
⟶
MgSO₄Crystalline solid + Co(OH)₂Crystalline solidpink, precipitated, aged

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard entropy of reaction Δ_rS° J · K⁻¹ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	–	−12.9	–	–
per 1 mol of Cobalt(II) sulfate	–	−12.9	–	–
per 1 mol of Magnesium hydroxide	–	−12.9	–	–
per 1 mol of Magnesium sulfate	–	−12.9	–	–
per 1 mol of Cobalt(II) hydroxide	–	−12.9	–	–

Changes in standard condition (4)

Reaction of cobalt(II) sulfate and magnesium hydroxide: CoSO₄Crystalline solid + Mg(OH)₂Amorphous solidprecipitated
⟶
MgSO₄Crystalline solid + Co(OH)₂Crystalline solidblue, precipitated

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard entropy of reaction Δ_rS° J · K⁻¹ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	–	–	–	–
per 1 mol of Cobalt(II) sulfate	–	–	–	–
per 1 mol of Magnesium hydroxide	–	–	–	–
per 1 mol of Magnesium sulfate	–	–	–	–
per 1 mol of Cobalt(II) hydroxide	–	–	–	–

Changes in standard condition (5)

Reaction of cobalt(II) sulfate and magnesium hydroxide: CoSO₄Crystalline solid + Mg(OH)₂Amorphous solidprecipitated
⟶
MgSO₄Crystalline solid + Co(OH)₂Crystalline solidpink, precipitated

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard entropy of reaction Δ_rS° J · K⁻¹ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	−15.8	–	–	–
per 1 mol of Cobalt(II) sulfate	−15.8	–	–	–
per 1 mol of Magnesium hydroxide	−15.8	–	–	–
per 1 mol of Magnesium sulfate	−15.8	–	–	–
per 1 mol of Cobalt(II) hydroxide	−15.8	–	–	–

Changes in standard condition (6)

Reaction of cobalt(II) sulfate and magnesium hydroxide: CoSO₄Crystalline solid + Mg(OH)₂Amorphous solidprecipitated
⟶
MgSO₄Crystalline solid + Co(OH)₂Crystalline solidpink, precipitated, aged

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard entropy of reaction Δ_rS° J · K⁻¹ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	–	–	–	–
per 1 mol of Cobalt(II) sulfate	–	–	–	–
per 1 mol of Magnesium hydroxide	–	–	–	–
per 1 mol of Magnesium sulfate	–	–	–	–
per 1 mol of Cobalt(II) hydroxide	–	–	–	–

Changes in aqueous solution (1)

Reaction of cobalt(II) sulfate and magnesium hydroxide ◆ Δ_rG −5.4 kJ/mol K 8.83 × 10⁰ pK −0.95: CoSO₄Crystalline solid + Mg(OH)₂Crystalline solid
⟶
MgSO₄Ionized aqueous solution + Co(OH)₂Un-ionized aqueous solution

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard entropy of reaction Δ_rS° J · K⁻¹ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	–	−5.4	–	–
per 1 mol of Cobalt(II) sulfate	–	−5.4	–	–
per 1 mol of Magnesium hydroxide	–	−5.4	–	–
per 1 mol of Magnesium sulfate	–	−5.4	–	–
per 1 mol of Cobalt(II) hydroxide	–	−5.4	–	–

Changes in aqueous solution (2)

Reaction of cobalt(II) sulfate and magnesium hydroxide ◆ Δ_rG −33.8 kJ/mol K 8.35 × 10⁵ pK −5.92: CoSO₄Crystalline solid + Mg(OH)₂Crystalline solid
⟶
MgSO₄Ionized aqueous solution + Co(OH)₂Crystalline solidblue, precipitated

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard entropy of reaction Δ_rS° J · K⁻¹ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	–	−33.8	–	–
per 1 mol of Cobalt(II) sulfate	–	−33.8	–	–
per 1 mol of Magnesium hydroxide	–	−33.8	–	–
per 1 mol of Magnesium sulfate	–	−33.8	–	–
per 1 mol of Cobalt(II) hydroxide	–	−33.8	–	–

Changes in aqueous solution (3)

Reaction of cobalt(II) sulfate and magnesium hydroxide ◆ Δ_rG −38.0 kJ/mol K 4.54 × 10⁶ pK −6.66: CoSO₄Crystalline solid + Mg(OH)₂Crystalline solid
⟶
MgSO₄Ionized aqueous solution + Co(OH)₂Crystalline solidpink, precipitated

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard entropy of reaction Δ_rS° J · K⁻¹ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	−103.0	−38.0	−220	–
per 1 mol of Cobalt(II) sulfate	−103.0	−38.0	−220	–
per 1 mol of Magnesium hydroxide	−103.0	−38.0	−220	–
per 1 mol of Magnesium sulfate	−103.0	−38.0	−220	–
per 1 mol of Cobalt(II) hydroxide	−103.0	−38.0	−220	–

Changes in aqueous solution (4)

Reaction of cobalt(II) sulfate and magnesium hydroxide ◆ Δ_rG −41.8 kJ/mol K 2.10 × 10⁷ pK −7.32: CoSO₄Crystalline solid + Mg(OH)₂Crystalline solid
⟶
MgSO₄Ionized aqueous solution + Co(OH)₂Crystalline solidpink, precipitated, aged

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard entropy of reaction Δ_rS° J · K⁻¹ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	–	−41.8	–	–
per 1 mol of Cobalt(II) sulfate	–	−41.8	–	–
per 1 mol of Magnesium hydroxide	–	−41.8	–	–
per 1 mol of Magnesium sulfate	–	−41.8	–	–
per 1 mol of Cobalt(II) hydroxide	–	−41.8	–	–

Changes in aqueous solution (5)

Reaction of cobalt(II) sulfate and magnesium hydroxide ◆ Δ_rG −18.1 kJ/mol K 1.48 × 10³ pK −3.17: CoSO₄Crystalline solid + Mg(OH)₂Crystalline solid
⟶
MgSO₄Un-ionized aqueous solution + Co(OH)₂Un-ionized aqueous solution

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard entropy of reaction Δ_rS° J · K⁻¹ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	–	−18.1	–	–
per 1 mol of Cobalt(II) sulfate	–	−18.1	–	–
per 1 mol of Magnesium hydroxide	–	−18.1	–	–
per 1 mol of Magnesium sulfate	–	−18.1	–	–
per 1 mol of Cobalt(II) hydroxide	–	−18.1	–	–

Changes in aqueous solution (6)

Reaction of cobalt(II) sulfate and magnesium hydroxide ◆ Δ_rG −46.5 kJ/mol K 1.40 × 10⁸ pK −8.15: CoSO₄Crystalline solid + Mg(OH)₂Crystalline solid
⟶
MgSO₄Un-ionized aqueous solution + Co(OH)₂Crystalline solidblue, precipitated

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard entropy of reaction Δ_rS° J · K⁻¹ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	–	−46.5	–	–
per 1 mol of Cobalt(II) sulfate	–	−46.5	–	–
per 1 mol of Magnesium hydroxide	–	−46.5	–	–
per 1 mol of Magnesium sulfate	–	−46.5	–	–
per 1 mol of Cobalt(II) hydroxide	–	−46.5	–	–

Changes in aqueous solution (7)

Reaction of cobalt(II) sulfate and magnesium hydroxide ◆ Δ_rG −50.7 kJ/mol K 7.63 × 10⁸ pK −8.88: CoSO₄Crystalline solid + Mg(OH)₂Crystalline solid
⟶
MgSO₄Un-ionized aqueous solution + Co(OH)₂Crystalline solidpink, precipitated

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard entropy of reaction Δ_rS° J · K⁻¹ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	−82.9	−50.7	−109	–
per 1 mol of Cobalt(II) sulfate	−82.9	−50.7	−109	–
per 1 mol of Magnesium hydroxide	−82.9	−50.7	−109	–
per 1 mol of Magnesium sulfate	−82.9	−50.7	−109	–
per 1 mol of Cobalt(II) hydroxide	−82.9	−50.7	−109	–

Changes in aqueous solution (8)

Reaction of cobalt(II) sulfate and magnesium hydroxide ◆ Δ_rG −54.5 kJ/mol K 3.53 × 10⁹ pK −9.55: CoSO₄Crystalline solid + Mg(OH)₂Crystalline solid
⟶
MgSO₄Un-ionized aqueous solution + Co(OH)₂Crystalline solidpink, precipitated, aged

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard entropy of reaction Δ_rS° J · K⁻¹ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	–	−54.5	–	–
per 1 mol of Cobalt(II) sulfate	–	−54.5	–	–
per 1 mol of Magnesium hydroxide	–	−54.5	–	–
per 1 mol of Magnesium sulfate	–	−54.5	–	–
per 1 mol of Cobalt(II) hydroxide	–	−54.5	–	–

Changes in aqueous solution (9)

Reaction of cobalt(II) sulfate and magnesium hydroxide: CoSO₄Crystalline solid + Mg(OH)₂Amorphous solidprecipitated
⟶
MgSO₄Ionized aqueous solution + Co(OH)₂Un-ionized aqueous solution

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard entropy of reaction Δ_rS° J · K⁻¹ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	–	–	–	–
per 1 mol of Cobalt(II) sulfate	–	–	–	–
per 1 mol of Magnesium hydroxide	–	–	–	–
per 1 mol of Magnesium sulfate	–	–	–	–
per 1 mol of Cobalt(II) hydroxide	–	–	–	–

Changes in aqueous solution (10)

Reaction of cobalt(II) sulfate and magnesium hydroxide: CoSO₄Crystalline solid + Mg(OH)₂Amorphous solidprecipitated
⟶
MgSO₄Ionized aqueous solution + Co(OH)₂Crystalline solidblue, precipitated

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard entropy of reaction Δ_rS° J · K⁻¹ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	–	–	–	–
per 1 mol of Cobalt(II) sulfate	–	–	–	–
per 1 mol of Magnesium hydroxide	–	–	–	–
per 1 mol of Magnesium sulfate	–	–	–	–
per 1 mol of Cobalt(II) hydroxide	–	–	–	–

Changes in aqueous solution (11)

Reaction of cobalt(II) sulfate and magnesium hydroxide: CoSO₄Crystalline solid + Mg(OH)₂Amorphous solidprecipitated
⟶
MgSO₄Ionized aqueous solution + Co(OH)₂Crystalline solidpink, precipitated

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard entropy of reaction Δ_rS° J · K⁻¹ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	−107.0	–	–	–
per 1 mol of Cobalt(II) sulfate	−107.0	–	–	–
per 1 mol of Magnesium hydroxide	−107.0	–	–	–
per 1 mol of Magnesium sulfate	−107.0	–	–	–
per 1 mol of Cobalt(II) hydroxide	−107.0	–	–	–

Changes in aqueous solution (12)

Reaction of cobalt(II) sulfate and magnesium hydroxide: CoSO₄Crystalline solid + Mg(OH)₂Amorphous solidprecipitated
⟶
MgSO₄Ionized aqueous solution + Co(OH)₂Crystalline solidpink, precipitated, aged

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard entropy of reaction Δ_rS° J · K⁻¹ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	–	–	–	–
per 1 mol of Cobalt(II) sulfate	–	–	–	–
per 1 mol of Magnesium hydroxide	–	–	–	–
per 1 mol of Magnesium sulfate	–	–	–	–
per 1 mol of Cobalt(II) hydroxide	–	–	–	–

Changes in aqueous solution (13)

Reaction of cobalt(II) sulfate and magnesium hydroxide: CoSO₄Crystalline solid + Mg(OH)₂Amorphous solidprecipitated
⟶
MgSO₄Un-ionized aqueous solution + Co(OH)₂Un-ionized aqueous solution

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard entropy of reaction Δ_rS° J · K⁻¹ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	–	–	–	–
per 1 mol of Cobalt(II) sulfate	–	–	–	–
per 1 mol of Magnesium hydroxide	–	–	–	–
per 1 mol of Magnesium sulfate	–	–	–	–
per 1 mol of Cobalt(II) hydroxide	–	–	–	–

Changes in aqueous solution (14)

Reaction of cobalt(II) sulfate and magnesium hydroxide: CoSO₄Crystalline solid + Mg(OH)₂Amorphous solidprecipitated
⟶
MgSO₄Un-ionized aqueous solution + Co(OH)₂Crystalline solidblue, precipitated

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard entropy of reaction Δ_rS° J · K⁻¹ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	–	–	–	–
per 1 mol of Cobalt(II) sulfate	–	–	–	–
per 1 mol of Magnesium hydroxide	–	–	–	–
per 1 mol of Magnesium sulfate	–	–	–	–
per 1 mol of Cobalt(II) hydroxide	–	–	–	–

Changes in aqueous solution (15)

Reaction of cobalt(II) sulfate and magnesium hydroxide: CoSO₄Crystalline solid + Mg(OH)₂Amorphous solidprecipitated
⟶
MgSO₄Un-ionized aqueous solution + Co(OH)₂Crystalline solidpink, precipitated

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard entropy of reaction Δ_rS° J · K⁻¹ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	−86.9	–	–	–
per 1 mol of Cobalt(II) sulfate	−86.9	–	–	–
per 1 mol of Magnesium hydroxide	−86.9	–	–	–
per 1 mol of Magnesium sulfate	−86.9	–	–	–
per 1 mol of Cobalt(II) hydroxide	−86.9	–	–	–

Changes in aqueous solution (16)

Reaction of cobalt(II) sulfate and magnesium hydroxide: CoSO₄Crystalline solid + Mg(OH)₂Amorphous solidprecipitated
⟶
MgSO₄Un-ionized aqueous solution + Co(OH)₂Crystalline solidpink, precipitated, aged

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard entropy of reaction Δ_rS° J · K⁻¹ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	–	–	–	–
per 1 mol of Cobalt(II) sulfate	–	–	–	–
per 1 mol of Magnesium hydroxide	–	–	–	–
per 1 mol of Magnesium sulfate	–	–	–	–
per 1 mol of Cobalt(II) hydroxide	–	–	–	–

Thermodynamic data of reactants

Chemical formula	Standard enthalpy of formation Δ_fH° kJ · mol⁻¹	Standard Gibbs energy of formation Δ_fG° kJ · mol⁻¹	Standard molar entropy S° J · K⁻¹ · mol⁻¹	Standard molar heat capacity at constant pressure C_p° J · K⁻¹ · mol⁻¹
CoSO₄ (cr)	-888.3^[1]	-782.3^[1]	118.0^[1]	–
CoSO₄ (ai)	-967.3^[1]	-799.1^[1]	-92^[1]	–
CoSO₄ (cr) 6 hydrate	-2683.6^[1]	-2235.36^[1]	367.61^[1]	353.38^[1]
CoSO₄ (cr) 7 hydrate	-2979.93^[1]	-2473.42^[1]	406.06^[1]	390.49^[1]
Mg(OH)₂ (cr)	-924.54^[1]	-833.51^[1]	63.18^[1]	77.03^[1]
Mg(OH)₂ (am) precipitated	-920.5^[1]	–	–	–
Mg(OH)₂ (g)	-561^[1]	–	–	–
Mg(OH)₂ (ai)	-926.84^[1]	-769.4^[1]	-159.4^[1]	–

* (cr):Crystalline solid, (ai):Ionized aqueous solution, (am):Amorphous solid, (g):Gas

Thermodynamic data of products

Chemical formula	Standard enthalpy of formation Δ_fH° kJ · mol⁻¹	Standard Gibbs energy of formation Δ_fG° kJ · mol⁻¹	Standard molar entropy S° J · K⁻¹ · mol⁻¹	Standard molar heat capacity at constant pressure C_p° J · K⁻¹ · mol⁻¹
MgSO₄ (cr)	-1284.9^[1]	-1170.6^[1]	91.6^[1]	96.48^[1]
MgSO₄ (ai)	-1376.12^[1]	-1199.5^[1]	-118.0^[1]	–
MgSO₄ (ao)	-1356.0^[1]	-1212.21^[1]	-7.1^[1]	–
MgSO₄ (cr) 1 hydrate	-1602.1^[1]	-1428.7^[1]	126.4^[1]	–
MgSO₄ (am) 1 hydrate	-1574.9^[1]	-1404.9^[1]	138.1^[1]	–
MgSO₄ (cr) 2 hydrate	-1896.2^[1]	–	–	–
MgSO₄ (cr) 4 hydrate	-2496.6^[1]	–	–	–
MgSO₄ (cr) 6 hydrate	-3087.0^[1]	-2631.8^[1]	348.1^[1]	348.11^[1]
MgSO₄ (cr) 7 hydrate	-3388.71^[1]	-2871.5^[1]	372^[1]	–
Co(OH)₂ (cr) blue, precipitated	–	-450.1^[1]	–	–
Co(OH)₂ (cr) pink, precipitated	-539.7^[1]	-454.3^[1]	79^[1]	–
Co(OH)₂ (cr) pink, precipitated, aged	–	-458.1^[1]	–	–
Co(OH)₂ (ai)	-518.0^[1]	-369.0^[1]	-134^[1]	–
Co(OH)₂ (ao)	–	-421.7^[1]	–	–

* (cr):Crystalline solid, (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution, (am):Amorphous solid

References

List of references

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
https://doi.org/10.18434/M32124
National Institute of Standards and Technology (NIST)
Citation list

Δ_rG	−4.9 kJ/mol
K	7.22 × 10⁰
pK	−0.86

Δ_rG	−9.1 kJ/mol
K	3.93 × 10¹
pK	−1.59

Δ_rG	−12.9 kJ/mol
K	1.82 × 10²
pK	−2.26

Δ_rG	−5.4 kJ/mol
K	8.83 × 10⁰
pK	−0.95

CoSO4 + Mg(OH)2 → MgSO4 + Co(OH)2