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Al2(SO4)3 + 3CuF2 💧→ 2AlF3↓ + 3CuSO4

Al₂(SO₄)₃ + 3CuF₂ 💧→ 2AlF₃↓ + 3CuSO₄

Last updated: June 13, 2022

Reaction of aluminium sulfate and copper(II) fluoride: Al₂(SO₄)₃Aluminium sulfate + 3CuF₂Copper(II) fluoride
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2AlF₃↓Aluminium fluoride + 3CuSO₄Copper(II) sulfate

The reaction of aluminium sulfate and copper(II) fluoride yields aluminium fluoride and copper(II) sulfate. This reaction is an acid-base reaction and is classified as follows:

Precipitation reaction

Table of contents

Reaction data

Reactants

Chemical formula	Name	Coefficient	Type	Type in general equation
Al₂(SO₄)₃	Aluminium sulfate	1	Lewis acid	Very soluble in water
CuF₂	Copper(II) fluoride	3	Lewis base	Soluble in water

Products

Chemical formula	Name	Coefficient	Type	Type in general equation
AlF₃	Aluminium fluoride	2	Lewis conjugate	Slightly soluble in water
CuSO₄	Copper(II) sulfate	3	Non-redox product	–

Thermodynamic changes

Changes in standard condition

Reaction of aluminium sulfate and copper(II) fluoride: Al₂(SO₄)₃Crystalline solid + 3CuF₂Crystalline solid
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2AlF₃↓Crystalline solid + 3CuSO₄Crystalline solid

	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	−253.3	–	–	–
per 1 mol of Aluminium sulfate	−253.3	–	–	–
per 1 mol of Copper(II) fluoride	−84.43	–	–	–
per 1 mol of Aluminium fluoride	−126.7	–	–	–
per 1 mol of Copper(II) sulfate	−84.43	–	–	–

Changes in aqueous solution (1)

Reaction of aluminium sulfate and copper(II) fluoride: Al₂(SO₄)₃Aqueous solution + 3CuF₂Crystalline solid
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2AlF₃↓Crystalline solid + 3CuSO₄Un-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 Aluminium sulfate	–	–	–	–
per 1 mol of Copper(II) fluoride	–	–	–	–
per 1 mol of Aluminium fluoride	–	–	–	–
per 1 mol of Copper(II) sulfate	–	–	–	–

Changes in aqueous solution (2)

Reaction of aluminium sulfate and copper(II) fluoride: Al₂(SO₄)₃Aqueous solution + 3CuF₂Crystalline solid
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2AlF₃↓Crystalline solid + 3CuSO₄Crystalline solid

	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	80.6	–	–	–
per 1 mol of Aluminium sulfate	80.6	–	–	–
per 1 mol of Copper(II) fluoride	26.9	–	–	–
per 1 mol of Aluminium fluoride	40.3	–	–	–
per 1 mol of Copper(II) sulfate	26.9	–	–	–

Changes in aqueous solution (3)

Reaction of aluminium sulfate and copper(II) fluoride: Al₂(SO₄)₃Ionized aqueous solution + 3CuF₂Crystalline solid
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2AlF₃↓Crystalline solid + 3CuSO₄Un-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 Aluminium sulfate	–	–	–	–
per 1 mol of Copper(II) fluoride	–	–	–	–
per 1 mol of Aluminium fluoride	–	–	–	–
per 1 mol of Copper(II) sulfate	–	–	–	–

Changes in aqueous solution (4)

Reaction of aluminium sulfate and copper(II) fluoride: Al₂(SO₄)₃Ionized aqueous solution + 3CuF₂Crystalline solid
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2AlF₃↓Crystalline solid + 3CuSO₄Crystalline solid

	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	97	–	–	–
per 1 mol of Aluminium sulfate	97	–	–	–
per 1 mol of Copper(II) fluoride	32	–	–	–
per 1 mol of Aluminium fluoride	49	–	–	–
per 1 mol of Copper(II) sulfate	32	–	–	–

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
Al₂(SO₄)₃ (cr)	-3440.84^[1]	-3099.94^[1]	239.3^[1]	259.41^[1]
Al₂(SO₄)₃ (ai)	-3791^[1]	-3205^[1]	-583.2^[1]	–
Al₂(SO₄)₃ (aq)	-3774.8^[1]	–	–	–
Al₂(SO₄)₃ (cr) 6 hydrate	-5311.71^[1]	-4622.08^[1]	469.0^[1]	492.9^[1]
Al₂(SO₄)₃ (cr) 18 hydrate	-8878.9^[1]	–	–	–
CuF₂ (cr)	-542.7^[1]	–	–	–
CuF₂ (cr) 2 hydrate	–	-981.4^[1]	–	–

* (cr):Crystalline solid, (ai):Ionized aqueous solution, (aq):Aqueous solution

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
AlF₃ (cr)	-1504.1^[1]	-1425.0^[1]	66.44^[1]	75.10^[1]
AlF₃ (g)	-1204.6^[1]	-1188.2^[1]	277.1^[1]	62.63^[1]
AlF₃ (ai)	-1531^[1]	-1322^[1]	-363.2^[1]	–
AlF₃ (ao)	-1519^[1]	-1414^[1]	-25^[1]	–
CuSO₄ (cr)	-771.36^[1]	-661.8^[1]	109^[1]	100.0^[1]
CuSO₄ (ai)	-844.50^[1]	-679.04^[1]	-79.5^[1]	–
CuSO₄ (ao)	–	-692.18^[1]	–	–
CuSO₄ (cr) 1 hydrate	-1085.83^[1]	-918.11^[1]	146.0^[1]	134^[1]
CuSO₄ (cr) 3 hydrate	-1684.31^[1]	-1399.96^[1]	221.3^[1]	205^[1]
CuSO₄ (cr) 5 hydrate	-2279.65^[1]	-1879.745^[1]	300.4^[1]	280^[1]

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

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

Al2(SO4)3 + 3CuF2 💧→ 2AlF3↓ + 3CuSO4

Reaction data

Chemical equation

General equation

Oxidation state of each atom