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BaI2 + ZnSO4 💧→ BaSO4↓ + ZnI2

BaI₂ + ZnSO₄ 💧→ BaSO₄↓ + ZnI₂

Last updated: June 13, 2022

Reaction of barium iodide and zinc sulfate: BaI₂Barium iodide + ZnSO₄Zinc sulfate
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BaSO₄↓Barium sulfate + ZnI₂Zinc iodide

The reaction of barium iodide and zinc sulfate yields barium sulfate and zinc iodide. 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
BaI₂	Barium iodide	1	Lewis acid	Very soluble in water
ZnSO₄	Zinc sulfate	1	Lewis base	Very soluble in water

Products

Chemical formula	Name	Coefficient	Type	Type in general equation
BaSO₄	Barium sulfate	1	Lewis conjugate	Insoluble in water
ZnI₂	Zinc iodide	1	Non-redox product	–

Thermodynamic changes

Changes in standard condition (1)

Reaction of barium iodide and zinc sulfate: BaI₂Crystalline solid + ZnSO₄Crystalline solid
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BaSO₄↓Crystalline solid + ZnI₂Crystalline 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	−96.3	–	–	–
per 1 mol of Barium iodide	−96.3	–	–	–
per 1 mol of Zinc sulfate	−96.3	–	–	–
per 1 mol of Barium sulfate	−96.3	–	–	–
per 1 mol of Zinc iodide	−96.3	–	–	–

Changes in standard condition (2)

Reaction of barium iodide and zinc sulfate: BaI₂Crystalline solid + ZnSO₄Crystalline solid
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BaSO₄↓Crystalline solidprecipitated + ZnI₂Crystalline 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	−89.6	–	–	–
per 1 mol of Barium iodide	−89.6	–	–	–
per 1 mol of Zinc sulfate	−89.6	–	–	–
per 1 mol of Barium sulfate	−89.6	–	–	–
per 1 mol of Zinc iodide	−89.6	–	–	–

Changes in aqueous solution (1)

Reaction of barium iodide and zinc sulfate ◆ Δ_rG 13.3 kJ/mol K 0.47 × 10⁻² pK 2.33: BaI₂Ionized aqueous solution + ZnSO₄Un-ionized aqueous solution
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BaSO₄↓Ionized aqueous solution + ZnI₂Ionized 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	1286.8	13.3	−97.0	–
per 1 mol of Barium iodide	1286.8	13.3	−97.0	–
per 1 mol of Zinc sulfate	1286.8	13.3	−97.0	–
per 1 mol of Barium sulfate	1286.8	13.3	−97.0	–
per 1 mol of Zinc iodide	1286.8	13.3	−97.0	–

Changes in aqueous solution (2)

Reaction of barium iodide and zinc sulfate ◆ Δ_rG 22.9 kJ/mol K 0.97 × 10⁻⁴ pK 4.01: BaI₂Ionized aqueous solution + ZnSO₄Un-ionized aqueous solution
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BaSO₄↓Ionized aqueous solution + ZnI₂Un-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	–	22.9	–	–
per 1 mol of Barium iodide	–	22.9	–	–
per 1 mol of Zinc sulfate	–	22.9	–	–
per 1 mol of Barium sulfate	–	22.9	–	–
per 1 mol of Zinc iodide	–	22.9	–	–

Changes in aqueous solution (3)

Reaction of barium iodide and zinc sulfate ◆ Δ_rG 0.01 kJ/mol K 1.00 × 10⁰ pK 0.00: BaI₂Ionized aqueous solution + ZnSO₄Ionized aqueous solution
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BaSO₄↓Ionized aqueous solution + ZnI₂Ionized aqueous solution

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	1302.22	0.01	–
per 1 mol of Barium iodide	1302.22	0.0100	–
per 1 mol of Zinc sulfate	1302.22	0.0100	–
per 1 mol of Barium sulfate	1302.22	0.0100	–
per 1 mol of Zinc iodide	1302.22	0.0100	–

Changes in aqueous solution (4)

Reaction of barium iodide and zinc sulfate ◆ Δ_rG 9.6 kJ/mol K 0.21 × 10⁻¹ pK 1.68: BaI₂Ionized aqueous solution + ZnSO₄Ionized aqueous solution
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BaSO₄↓Ionized aqueous solution + ZnI₂Un-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	–	9.6	–	–
per 1 mol of Barium iodide	–	9.6	–	–
per 1 mol of Zinc sulfate	–	9.6	–	–
per 1 mol of Barium sulfate	–	9.6	–	–
per 1 mol of Zinc iodide	–	9.6	–	–

Changes in aqueous solution (5)

Reaction of barium iodide and zinc sulfate ◆ Δ_rG 13.3 kJ/mol K 0.47 × 10⁻² pK 2.33: BaI₂Ionized aqueous solution + ZnSO₄Un-ionized aqueous solution
💧
⟶
BaSO₄↓Ionized aqueous solution + ZnI₂Ionized 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	1286.8	13.3	−97.0	–
per 1 mol of Barium iodide	1286.8	13.3	−97.0	–
per 1 mol of Zinc sulfate	1286.8	13.3	−97.0	–
per 1 mol of Barium sulfate	1286.8	13.3	−97.0	–
per 1 mol of Zinc iodide	1286.8	13.3	−97.0	–

Changes in aqueous solution (6)

Reaction of barium iodide and zinc sulfate ◆ Δ_rG 22.9 kJ/mol K 0.97 × 10⁻⁴ pK 4.01: BaI₂Ionized aqueous solution + ZnSO₄Un-ionized aqueous solution
💧
⟶
BaSO₄↓Ionized aqueous solution + ZnI₂Un-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	–	22.9	–	–
per 1 mol of Barium iodide	–	22.9	–	–
per 1 mol of Zinc sulfate	–	22.9	–	–
per 1 mol of Barium sulfate	–	22.9	–	–
per 1 mol of Zinc iodide	–	22.9	–	–

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
BaI₂ (cr)	-602.1^[1]	–	–	–
BaI₂ (g)	-326^[1]	-377^[1]	343^[1]	61.5^[1]
BaI₂ (ai)	-648.02^[1]	-663.92^[1]	232.2^[1]	–
BaI₂ (cr) 1 hydrate	-919.2^[1]	–	–	–
BaI₂ (cr) 2 hydrate	-1216.7^[1]	–	–	–
BaI₂ (cr) 2.5 hydrate	-1363.6^[1]	–	–	–
BaI₂ (cr) 7 hydrate	-2676.5^[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]

* (cr):Crystalline solid, (g):Gas, (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
BaSO₄ (cr)	-1473.2^[1]	-1362.2^[1]	132.2^[1]	101.75^[1]
BaSO₄ (cr) precipitated	-1466.5^[1]	–	–	–
BaSO₄ (ai)	-144.691^[1]	-1305.30^[1]	29.7^[1]	–
ZnI₂ (cr)	-208.03^[1]	-208.95^[1]	161.1^[1]	–
ZnI₂ (ai)	-264.26^[1]	-250.20^[1]	110.5^[1]	-238^[1]
ZnI₂ (ao)	–	-240.6^[1]	–	–

* (cr):Crystalline solid, (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

Δ_rG	13.3 kJ/mol
K	0.47 × 10⁻²
pK	2.33

Δ_rG	22.9 kJ/mol
K	0.97 × 10⁻⁴
pK	4.01

Δ_rG	0.01 kJ/mol
K	1.00 × 10⁰
pK	0.00

Δ_rG	9.6 kJ/mol
K	0.21 × 10⁻¹
pK	1.68

BaI2 + ZnSO4 💧→ BaSO4↓ + ZnI2