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Chemical reactions
2AgNO3 + ZnI2 💧→ 2AgI↓ + Zn(NO3)2

2AgNO₃ + ZnI₂ 💧→ 2AgI↓ + Zn(NO₃)₂

Last updated: June 13, 2022

Reaction of silver(I) nitrate and zinc iodide: 2AgNO₃Silver(I) nitrate + ZnI₂Zinc iodide
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2AgI↓Silver(I) iodide + Zn(NO₃)₂Zinc nitrate

The reaction of silver(I) nitrate and zinc iodide yields silver(I) iodide and zinc nitrate. 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
AgNO₃	Silver(I) nitrate	2	Lewis acid	Very soluble in water
ZnI₂	Zinc iodide	1	Lewis base	Very soluble in water

Products

Chemical formula	Name	Coefficient	Type	Type in general equation
AgI	Silver(I) iodide	2	Lewis conjugate	Insoluble in water
Zn(NO₃)₂	Zinc nitrate	1	Non-redox product	–

Thermodynamic changes

Changes in standard condition

Reaction of silver(I) nitrate and zinc iodide: 2AgNO₃Crystalline solid + ZnI₂Crystalline solid
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2AgI↓Crystalline solid + Zn(NO₃)₂Crystalline 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	−150.6	–	–	–
per 1 mol of Silver(I) nitrate	−75.30	–	–	–
per 1 mol of Zinc iodide	−150.6	–	–	–
per 1 mol of Silver(I) iodide	−75.30	–	–	–
per 1 mol of Zinc nitrate	−150.6	–	–	–

Changes in aqueous solution (1)

Reaction of silver(I) nitrate and zinc iodide ◆ Δ_rG −0.01 kJ/mol K 1.00 × 10⁰ pK −0.00: 2AgNO₃Ionized aqueous solution + ZnI₂Ionized aqueous solution
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2AgI↓Ionized aqueous solution + Zn(NO₃)₂Ionized 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	0.01	−0.01	1
per 1 mol of Silver(I) nitrate	0.00500	−0.00500	0.5
per 1 mol of Zinc iodide	0.0100	−0.0100	1
per 1 mol of Silver(I) iodide	0.00500	−0.00500	0.5
per 1 mol of Zinc nitrate	0.0100	−0.0100	1

Changes in aqueous solution (2)

Reaction of silver(I) nitrate and zinc iodide ◆ Δ_rG −75.3 kJ/mol K 1.56 × 10¹³ pK −13.19: 2AgNO₃Ionized aqueous solution + ZnI₂Ionized aqueous solution
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2AgI↓Un-ionized aqueous solution + Zn(NO₃)₂Ionized 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	–	−75.3	–	–
per 1 mol of Silver(I) nitrate	–	−37.6	–	–
per 1 mol of Zinc iodide	–	−75.3	–	–
per 1 mol of Silver(I) iodide	–	−37.6	–	–
per 1 mol of Zinc nitrate	–	−75.3	–	–

Changes in aqueous solution (3)

Reaction of silver(I) nitrate and zinc iodide ◆ Δ_rG −9.6 kJ/mol K 4.81 × 10¹ pK −1.68: 2AgNO₃Ionized aqueous solution + ZnI₂Un-ionized aqueous solution
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2AgI↓Ionized aqueous solution + Zn(NO₃)₂Ionized 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 Silver(I) nitrate	–	−4.8	–	–
per 1 mol of Zinc iodide	–	−9.6	–	–
per 1 mol of Silver(I) iodide	–	−4.8	–	–
per 1 mol of Zinc nitrate	–	−9.6	–	–

Changes in aqueous solution (4)

Reaction of silver(I) nitrate and zinc iodide ◆ Δ_rG −84.9 kJ/mol K 7.48 × 10¹⁴ pK −14.87: 2AgNO₃Ionized aqueous solution + ZnI₂Un-ionized aqueous solution
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2AgI↓Un-ionized aqueous solution + Zn(NO₃)₂Ionized 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	–	−84.9	–	–
per 1 mol of Silver(I) nitrate	–	−42.5	–	–
per 1 mol of Zinc iodide	–	−84.9	–	–
per 1 mol of Silver(I) iodide	–	−42.5	–	–
per 1 mol of Zinc nitrate	–	−84.9	–	–

Changes in aqueous solution (5)

Reaction of silver(I) nitrate and zinc iodide ◆ Δ_rG −3.35 kJ/mol K 3.86 × 10⁰ pK −0.59: 2AgNO₃Un-ionized aqueous solution + ZnI₂Ionized aqueous solution
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2AgI↓Ionized aqueous solution + Zn(NO₃)₂Ionized 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	–	−3.35	–	–
per 1 mol of Silver(I) nitrate	–	−1.68	–	–
per 1 mol of Zinc iodide	–	−3.35	–	–
per 1 mol of Silver(I) iodide	–	−1.68	–	–
per 1 mol of Zinc nitrate	–	−3.35	–	–

Changes in aqueous solution (6)

Reaction of silver(I) nitrate and zinc iodide ◆ Δ_rG −78.6 kJ/mol K 5.89 × 10¹³ pK −13.77: 2AgNO₃Un-ionized aqueous solution + ZnI₂Ionized aqueous solution
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2AgI↓Un-ionized aqueous solution + Zn(NO₃)₂Ionized 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	–	−78.6	–	–
per 1 mol of Silver(I) nitrate	–	−39.3	–	–
per 1 mol of Zinc iodide	–	−78.6	–	–
per 1 mol of Silver(I) iodide	–	−39.3	–	–
per 1 mol of Zinc nitrate	–	−78.6	–	–

Changes in aqueous solution (7)

Reaction of silver(I) nitrate and zinc iodide ◆ Δ_rG −13.0 kJ/mol K 1.89 × 10² pK −2.28: 2AgNO₃Un-ionized aqueous solution + ZnI₂Un-ionized aqueous solution
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2AgI↓Ionized aqueous solution + Zn(NO₃)₂Ionized 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	–	−13.0	–	–
per 1 mol of Silver(I) nitrate	–	−6.50	–	–
per 1 mol of Zinc iodide	–	−13.0	–	–
per 1 mol of Silver(I) iodide	–	−6.50	–	–
per 1 mol of Zinc nitrate	–	−13.0	–	–

Changes in aqueous solution (8)

Reaction of silver(I) nitrate and zinc iodide ◆ Δ_rG −88.2 kJ/mol K 2.83 × 10¹⁵ pK −15.45: 2AgNO₃Un-ionized aqueous solution + ZnI₂Un-ionized aqueous solution
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2AgI↓Un-ionized aqueous solution + Zn(NO₃)₂Ionized 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	–	−88.2	–	–
per 1 mol of Silver(I) nitrate	–	−44.1	–	–
per 1 mol of Zinc iodide	–	−88.2	–	–
per 1 mol of Silver(I) iodide	–	−44.1	–	–
per 1 mol of Zinc nitrate	–	−88.2	–	–

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
AgNO₃ (cr)	-124.39^[1]	-33.41^[1]	140.92^[1]	93.05^[1]
AgNO₃ (ai)	-101.80^[1]	-34.16^[1]	219.2^[1]	-64.9^[1]
AgNO₃ (ao)	–	-32.49^[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

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
AgI (cr)	-61.84^[1]	-66.19^[1]	115.5^[1]	56.82^[1]
AgI (ai)	50.38^[1]	25.52^[1]	184.1^[1]	-120.5^[1]
AgI (ao)	–	-12.1^[1]	–	–
Zn(NO₃)₂ (cr)	-483.7^[1]	–	–	–
Zn(NO₃)₂ (ai)	-568.61^[1]	-369.57^[1]	180.7^[1]	-126^[1]
Zn(NO₃)₂ (cr) 1 hydrate	-805.0^[1]	–	–	–
Zn(NO₃)₂ (cr) 2 hydrate	-1110.27^[1]	–	–	–
Zn(NO₃)₂ (cr) 4 hydrate	-1699.12^[1]	–	–	–
Zn(NO₃)₂ (cr) 6 hydrate	-2306.64^[1]	-1772.71^[1]	456.9^[1]	323.0^[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	−0.01 kJ/mol
K	1.00 × 10⁰
pK	−0.00

Δ_rG	−75.3 kJ/mol
K	1.56 × 10¹³
pK	−13.19

Δ_rG	−9.6 kJ/mol
K	4.81 × 10¹
pK	−1.68

Δ_rG	−84.9 kJ/mol
K	7.48 × 10¹⁴
pK	−14.87

2AgNO3 + ZnI2 💧→ 2AgI↓ + Zn(NO3)2