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ZnSO4 + 2Na[Al(OH)4] 💧→ Zn(OH)2↓ + 2Al(OH)3↓ + Na2SO4

ZnSO₄ + 2Na[Al(OH)₄] 💧→ Zn(OH)₂↓ + 2Al(OH)₃↓ + Na₂SO₄

Last updated: June 13, 2022

Reaction of zinc sulfate and sodium tetrahydroxydoaluminate: ZnSO₄Zinc sulfate + 2Na[Al(OH)₄]Sodium tetrahydroxydoaluminate
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⟶
Zn(OH)₂↓Zinc hydroxide + 2Al(OH)₃↓Aluminium hydroxide + Na₂SO₄Sodium sulfate

The reaction of zinc sulfate and sodium tetrahydroxydoaluminate yields zinc hydroxide, aluminium hydroxide, and sodium sulfate (Other reactions are here). 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
ZnSO₄	Zinc sulfate	1	Lewis acid	Very soluble in water
Na[Al(OH)₄]	Sodium tetrahydroxydoaluminate	2	Lewis base	Very soluble in water

Products

Chemical formula	Name	Coefficient	Type	Type in general equation
Zn(OH)₂	Zinc hydroxide	1	Lewis conjugate	Insoluble in water
Al(OH)₃	Aluminium hydroxide	2	Lewis conjugate	Insoluble in water
Na₂SO₄	Sodium sulfate	1	Non-redox product	–

Thermodynamic changes

Changes in standard condition (1)

Reaction of zinc sulfate and sodium tetrahydroxydoaluminate ◆ Δ_rG −364 kJ/mol K 5.89 × 10⁶³ pK −63.77: ZnSO₄Un-ionized aqueous solution + 2Na[Al(OH)₄]Ionized aqueous solution
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⟶
Zn(OH)₂↓Un-ionized aqueous solution + 2Al(OH)₃↓Crystalline solid + Na₂SO₄Ionized 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	–	−364	–	–
per 1 mol of Zinc sulfate	–	−364	–	–
per 1 mol of Sodium tetrahydroxydoaluminate	–	−182	–	–
per 1 mol of Zinc hydroxide	–	−364	–	–
per 1 mol of Aluminium hydroxide	–	−182	–	–
per 1 mol of Sodium sulfate	–	−364	–	–

Changes in standard condition (2)

Reaction of zinc sulfate and sodium tetrahydroxydoaluminate ◆ Δ_rG −395 kJ/mol K 1.59 × 10⁶⁹ pK −69.20: ZnSO₄Un-ionized aqueous solution + 2Na[Al(OH)₄]Ionized aqueous solution
💧
⟶
Zn(OH)₂↓Crystalline solidγ + 2Al(OH)₃↓Crystalline solid + Na₂SO₄Ionized 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	–	−395	–	–
per 1 mol of Zinc sulfate	–	−395	–	–
per 1 mol of Sodium tetrahydroxydoaluminate	–	−198	–	–
per 1 mol of Zinc hydroxide	–	−395	–	–
per 1 mol of Aluminium hydroxide	–	−198	–	–
per 1 mol of Sodium sulfate	–	−395	–	–

Changes in standard condition (3)

Reaction of zinc sulfate and sodium tetrahydroxydoaluminate ◆ Δ_rG −395 kJ/mol K 1.59 × 10⁶⁹ pK −69.20: ZnSO₄Un-ionized aqueous solution + 2Na[Al(OH)₄]Ionized aqueous solution
💧
⟶
Zn(OH)₂↓Crystalline solidβ + 2Al(OH)₃↓Crystalline solid + Na₂SO₄Ionized 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	−67	−395	33	–
per 1 mol of Zinc sulfate	−67	−395	33	–
per 1 mol of Sodium tetrahydroxydoaluminate	−34	−198	17	–
per 1 mol of Zinc hydroxide	−67	−395	33	–
per 1 mol of Aluminium hydroxide	−34	−198	17	–
per 1 mol of Sodium sulfate	−67	−395	33	–

Changes in standard condition (4)

Reaction of zinc sulfate and sodium tetrahydroxydoaluminate ◆ Δ_rG −396 kJ/mol K 2.38 × 10⁶⁹ pK −69.38: ZnSO₄Un-ionized aqueous solution + 2Na[Al(OH)₄]Ionized aqueous solution
💧
⟶
Zn(OH)₂↓Crystalline solidε + 2Al(OH)₃↓Crystalline solid + Na₂SO₄Ionized 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	−68	−396	33	–
per 1 mol of Zinc sulfate	−68	−396	33	–
per 1 mol of Sodium tetrahydroxydoaluminate	−34	−198	17	–
per 1 mol of Zinc hydroxide	−68	−396	33	–
per 1 mol of Aluminium hydroxide	−34	−198	17	–
per 1 mol of Sodium sulfate	−68	−396	33	–

Changes in standard condition (5)

Reaction of zinc sulfate and sodium tetrahydroxydoaluminate: ZnSO₄Un-ionized aqueous solution + 2Na[Al(OH)₄]Ionized aqueous solution
💧
⟶
Zn(OH)₂↓Crystalline solidprecipitated + 2Al(OH)₃↓Crystalline solid + Na₂SO₄Ionized 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	−67	–	–	–
per 1 mol of Zinc sulfate	−67	–	–	–
per 1 mol of Sodium tetrahydroxydoaluminate	−34	–	–	–
per 1 mol of Zinc hydroxide	−67	–	–	–
per 1 mol of Aluminium hydroxide	−34	–	–	–
per 1 mol of Sodium sulfate	−67	–	–	–

Changes in standard condition (6)

Reaction of zinc sulfate and sodium tetrahydroxydoaluminate ◆ Δ_rG −377 kJ/mol K 1.12 × 10⁶⁶ pK −66.05: ZnSO₄Ionized aqueous solution + 2Na[Al(OH)₄]Ionized aqueous solution
💧
⟶
Zn(OH)₂↓Un-ionized aqueous solution + 2Al(OH)₃↓Crystalline solid + Na₂SO₄Ionized 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	–	−377	–	–
per 1 mol of Zinc sulfate	–	−377	–	–
per 1 mol of Sodium tetrahydroxydoaluminate	–	−189	–	–
per 1 mol of Zinc hydroxide	–	−377	–	–
per 1 mol of Aluminium hydroxide	–	−189	–	–
per 1 mol of Sodium sulfate	–	−377	–	–

Changes in standard condition (7)

Reaction of zinc sulfate and sodium tetrahydroxydoaluminate ◆ Δ_rG −408 kJ/mol K 3.01 × 10⁷¹ pK −71.48: ZnSO₄Ionized aqueous solution + 2Na[Al(OH)₄]Ionized aqueous solution
💧
⟶
Zn(OH)₂↓Crystalline solidγ + 2Al(OH)₃↓Crystalline solid + Na₂SO₄Ionized 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	–	−408	–	–
per 1 mol of Zinc sulfate	–	−408	–	–
per 1 mol of Sodium tetrahydroxydoaluminate	–	−204	–	–
per 1 mol of Zinc hydroxide	–	−408	–	–
per 1 mol of Aluminium hydroxide	–	−204	–	–
per 1 mol of Sodium sulfate	–	−408	–	–

Changes in standard condition (8)

Reaction of zinc sulfate and sodium tetrahydroxydoaluminate ◆ Δ_rG −408 kJ/mol K 3.01 × 10⁷¹ pK −71.48: ZnSO₄Ionized aqueous solution + 2Na[Al(OH)₄]Ionized aqueous solution
💧
⟶
Zn(OH)₂↓Crystalline solidβ + 2Al(OH)₃↓Crystalline solid + Na₂SO₄Ionized 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	−51	−408	130	–
per 1 mol of Zinc sulfate	−51	−408	130	–
per 1 mol of Sodium tetrahydroxydoaluminate	−26	−204	65.0	–
per 1 mol of Zinc hydroxide	−51	−408	130	–
per 1 mol of Aluminium hydroxide	−26	−204	65.0	–
per 1 mol of Sodium sulfate	−51	−408	130	–

Changes in standard condition (9)

Reaction of zinc sulfate and sodium tetrahydroxydoaluminate ◆ Δ_rG −409 kJ/mol K 4.51 × 10⁷¹ pK −71.65: ZnSO₄Ionized aqueous solution + 2Na[Al(OH)₄]Ionized aqueous solution
💧
⟶
Zn(OH)₂↓Crystalline solidε + 2Al(OH)₃↓Crystalline solid + Na₂SO₄Ionized 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	−52	−409	130	–
per 1 mol of Zinc sulfate	−52	−409	130	–
per 1 mol of Sodium tetrahydroxydoaluminate	−26	−205	65.0	–
per 1 mol of Zinc hydroxide	−52	−409	130	–
per 1 mol of Aluminium hydroxide	−26	−205	65.0	–
per 1 mol of Sodium sulfate	−52	−409	130	–

Changes in standard condition (10)

Reaction of zinc sulfate and sodium tetrahydroxydoaluminate: ZnSO₄Ionized aqueous solution + 2Na[Al(OH)₄]Ionized aqueous solution
💧
⟶
Zn(OH)₂↓Crystalline solidprecipitated + 2Al(OH)₃↓Crystalline solid + Na₂SO₄Ionized 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	−51	–	–	–
per 1 mol of Zinc sulfate	−51	–	–	–
per 1 mol of Sodium tetrahydroxydoaluminate	−26	–	–	–
per 1 mol of Zinc hydroxide	−51	–	–	–
per 1 mol of Aluminium hydroxide	−26	–	–	–
per 1 mol of Sodium sulfate	−51	–	–	–

Changes in standard condition (11)

Reaction of zinc sulfate and sodium tetrahydroxydoaluminate ◆ Δ_rG −364 kJ/mol K 5.89 × 10⁶³ pK −63.77: ZnSO₄Un-ionized aqueous solution + 2Na[Al(OH)₄]Ionized aqueous solution
💧
⟶
Zn(OH)₂↓Un-ionized aqueous solution + 2Al(OH)₃↓Crystalline solid + Na₂SO₄Ionized 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	–	−364	–	–
per 1 mol of Zinc sulfate	–	−364	–	–
per 1 mol of Sodium tetrahydroxydoaluminate	–	−182	–	–
per 1 mol of Zinc hydroxide	–	−364	–	–
per 1 mol of Aluminium hydroxide	–	−182	–	–
per 1 mol of Sodium sulfate	–	−364	–	–

Changes in standard condition (12)

Reaction of zinc sulfate and sodium tetrahydroxydoaluminate ◆ Δ_rG −395 kJ/mol K 1.59 × 10⁶⁹ pK −69.20: ZnSO₄Un-ionized aqueous solution + 2Na[Al(OH)₄]Ionized aqueous solution
💧
⟶
Zn(OH)₂↓Crystalline solidγ + 2Al(OH)₃↓Crystalline solid + Na₂SO₄Ionized 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	–	−395	–	–
per 1 mol of Zinc sulfate	–	−395	–	–
per 1 mol of Sodium tetrahydroxydoaluminate	–	−198	–	–
per 1 mol of Zinc hydroxide	–	−395	–	–
per 1 mol of Aluminium hydroxide	–	−198	–	–
per 1 mol of Sodium sulfate	–	−395	–	–

Changes in standard condition (13)

Reaction of zinc sulfate and sodium tetrahydroxydoaluminate ◆ Δ_rG −395 kJ/mol K 1.59 × 10⁶⁹ pK −69.20: ZnSO₄Un-ionized aqueous solution + 2Na[Al(OH)₄]Ionized aqueous solution
💧
⟶
Zn(OH)₂↓Crystalline solidβ + 2Al(OH)₃↓Crystalline solid + Na₂SO₄Ionized 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	−67	−395	33	–
per 1 mol of Zinc sulfate	−67	−395	33	–
per 1 mol of Sodium tetrahydroxydoaluminate	−34	−198	17	–
per 1 mol of Zinc hydroxide	−67	−395	33	–
per 1 mol of Aluminium hydroxide	−34	−198	17	–
per 1 mol of Sodium sulfate	−67	−395	33	–

Changes in standard condition (14)

Reaction of zinc sulfate and sodium tetrahydroxydoaluminate ◆ Δ_rG −396 kJ/mol K 2.38 × 10⁶⁹ pK −69.38: ZnSO₄Un-ionized aqueous solution + 2Na[Al(OH)₄]Ionized aqueous solution
💧
⟶
Zn(OH)₂↓Crystalline solidε + 2Al(OH)₃↓Crystalline solid + Na₂SO₄Ionized 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	−68	−396	33	–
per 1 mol of Zinc sulfate	−68	−396	33	–
per 1 mol of Sodium tetrahydroxydoaluminate	−34	−198	17	–
per 1 mol of Zinc hydroxide	−68	−396	33	–
per 1 mol of Aluminium hydroxide	−34	−198	17	–
per 1 mol of Sodium sulfate	−68	−396	33	–

Changes in standard condition (15)

Reaction of zinc sulfate and sodium tetrahydroxydoaluminate: ZnSO₄Un-ionized aqueous solution + 2Na[Al(OH)₄]Ionized aqueous solution
💧
⟶
Zn(OH)₂↓Crystalline solidprecipitated + 2Al(OH)₃↓Crystalline solid + Na₂SO₄Ionized 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	−67	–	–	–
per 1 mol of Zinc sulfate	−67	–	–	–
per 1 mol of Sodium tetrahydroxydoaluminate	−34	–	–	–
per 1 mol of Zinc hydroxide	−67	–	–	–
per 1 mol of Aluminium hydroxide	−34	–	–	–
per 1 mol of Sodium sulfate	−67	–	–	–

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
ZnSO₄ (cr)	-982.8^[1]	-871.5^[1]	110.5^[1]	99.2^[1]
ZnSO₄ (ai)	-1063.15^[1]	-891.59^[1]	-92.0^[1]	-247^[1]
ZnSO₄ (ao)	-1047.7^[1]	-904.9^[1]	5.0^[1]	–
ZnSO₄ (cr) 1 hydrate	-1304.49^[1]	-1131.99^[1]	138.5^[1]	–
ZnSO₄ (cr) 6 hydrate	-2777.46^[1]	-2324.44^[1]	363.6^[1]	357.69^[1]
ZnSO₄ (cr) 7 hydrate	-3077.75^[1]	-2562.67^[1]	388.7^[1]	383.42^[1]
Na[Al(OH)₄] (ai)	-1742.6^[1]	-1567.2^[1]	161.9^[1]	–

* (cr):Crystalline solid, (ai):Ionized aqueous solution, (ao):Un-ionized 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
Zn(OH)₂ (cr) γ	–	-553.81^[1]	–	–
Zn(OH)₂ (cr) β	-641.91^[1]	-553.52^[1]	81.2^[1]	–
Zn(OH)₂ (cr) ε	-643.25^[1]	-555.07^[1]	81.6^[1]	72.4^[1]
Zn(OH)₂ (cr) precipitated	-642.2^[1]	–	–	–
Zn(OH)₂ (ai)	-613.88^[1]	-461.56^[1]	-133.5^[1]	-251^[1]
Zn(OH)₂ (ao)	–	-522.73^[1]	–	–
Al(OH)₃ (cr)	-1284^[2]	-1306^[2]	71^[2]	93.1^[2]
Al(OH)₃ (am)	-1276^[1]	–	–	–
Na₂SO₄ (cr) orthorhombic	-1387.08^[1]	-1270.16^[1]	149.58^[1]	128.20^[1]
Na₂SO₄ (cr) metastable	–	–	154.934^[1]	129.29^[1]
Na₂SO₄ (ai)	-1389.51^[1]	-1268.36^[1]	138.1^[1]	-201^[1]
Na₂SO₄ (cr) 10 hydrate	-4327.26^[1]	-3646.85^[1]	592.0^[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
2
James G. Speight (2017)
Lange's Handbook of Chemistry, 17th edition
https://www.accessengineeringlibrary.com/content/book/9781259586095
McGraw Hill Education
- Amazon
Citation list
- ^ Δ_fH°, -1284 kJ · mol⁻¹ - p.254
- ^ Δ_fG°, -1306 kJ · mol⁻¹ - p.254
- ^ S°, 71 J · K⁻¹ · mol⁻¹ - p.254
- ^ C_p°, 93.1 J · K⁻¹ · mol⁻¹ - p.254

Δ_rG	−364 kJ/mol
K	5.89 × 10⁶³
pK	−63.77

Δ_rG	−395 kJ/mol
K	1.59 × 10⁶⁹
pK	−69.20

Δ_rG	−395 kJ/mol
K	1.59 × 10⁶⁹
pK	−69.20

Δ_rG	−396 kJ/mol
K	2.38 × 10⁶⁹
pK	−69.38

ZnSO4 + 2Na[Al(OH)4] 💧→ Zn(OH)2↓ + 2Al(OH)3↓ + Na2SO4