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AgNO3 + NaI 💧→ AgI↓ + NaNO3

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Reaction of silver(I) nitrate and sodium iodide
AgNO3Silver(I) nitrate + NaISodium iodide
💧
⟶
AgI↓Silver(I) iodide + NaNO3Sodium nitrate

The reaction of silver(I) nitrate and sodium iodide yields silver(I) iodide and sodium nitrate. This reaction is an acid-base reaction and is classified as follows:

Table of contents
  1. 1Reaction data
  2. 2Thermodynamic changes
  3. 3References
  4. 4Related categories

Reaction data

Chemical equation

Reaction of silver(I) nitrate and sodium iodide
AgNO3Silver(I) nitrate + NaISodium iodide
💧
⟶
AgI↓Silver(I) iodide + NaNO3Sodium nitrate

General equation

Precipitation reaction
Miscible with water/Very soluble in water/Soluble in waterLewis acid + Miscible with water/Very soluble in water/Soluble in waterLewis base
💧
⟶
Insoluble in water/Very slightly soluble in water/Slightly soluble in waterLewis conjugate + Product(Non-redox product)

Oxidation state of each atom

Reaction of silver(I) nitrate and sodium iodide

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
AgNO3Silver(I) nitrate1
Lewis acid
Very soluble in water
NaISodium iodide1
Lewis base
Very soluble in water

Products

Chemical formulaNameCoefficientTypeType in general
equation
AgISilver(I) iodide1
Lewis conjugate
Insoluble in water
NaNO3Sodium nitrate1
Non-redox product
–

Thermodynamic changes

Changes in standard condition

Reaction of silver(I) nitrate and sodium iodide
◆
ΔrG−113.72 kJ/mol
K8.37 × 1019
pK−19.92
AgNO3Crystalline solid + NaICrystalline solid
💧
⟶
AgI↓Crystalline solid + NaNO3Crystalline solid
Standard enthalpy
of reaction
ΔrH°
kJ · mol−1		Standard
Gibbs energy
of reaction
ΔrG°
kJ · mol−1		Standard entropy
of reaction
ΔrS°
J · K−1 · mol−1		Standard heat
capacity of reaction
at constant pressure
ΔrCp°
J · K−1 · mol−1
per 1 mol of
Equation
−117.52−113.72−7.44.56
per 1 mol of
−117.52−113.72−7.44.56
per 1 mol of
−117.52−113.72−7.44.56
per 1 mol of
−117.52−113.72−7.44.56
per 1 mol of
−117.52−113.72−7.44.56

Changes in aqueous solution (1)

Reaction of silver(I) nitrate and sodium iodide
◆
ΔrG0.00 kJ/mol
K1.00 × 100
pK0.00
AgNO3Ionized aqueous solution + NaIIonized aqueous solution
💧
⟶
AgI↓Ionized aqueous solution + NaNO3Ionized aqueous solution
Standard enthalpy
of reaction
ΔrH°
kJ · mol−1		Standard
Gibbs energy
of reaction
ΔrG°
kJ · mol−1		Standard entropy
of reaction
ΔrS°
J · K−1 · mol−1		Standard heat
capacity of reaction
at constant pressure
ΔrCp°
J · K−1 · mol−1
per 1 mol of
Equation
0.010.000.00.0
per 1 mol of
0.01000.000.00.0
per 1 mol of
0.01000.000.00.0
per 1 mol of
0.01000.000.00.0
per 1 mol of
0.01000.000.00.0

Changes in aqueous solution (2)

Reaction of silver(I) nitrate and sodium iodide
◆
ΔrG−37.6 kJ/mol
K3.87 × 106
pK−6.59
AgNO3Ionized aqueous solution + NaIIonized aqueous solution
💧
⟶
AgI↓Un-ionized aqueous solution + NaNO3Ionized aqueous solution
Standard enthalpy
of reaction
ΔrH°
kJ · mol−1		Standard
Gibbs energy
of reaction
ΔrG°
kJ · mol−1		Standard entropy
of reaction
ΔrS°
J · K−1 · mol−1		Standard heat
capacity of reaction
at constant pressure
ΔrCp°
J · K−1 · mol−1
per 1 mol of
Equation
–−37.6––
per 1 mol of
–−37.6––
per 1 mol of
–−37.6––
per 1 mol of
–−37.6––
per 1 mol of
–−37.6––

Changes in aqueous solution (3)

Reaction of silver(I) nitrate and sodium iodide
◆
ΔrG−1.67 kJ/mol
K1.96 × 100
pK−0.29
AgNO3Un-ionized aqueous solution + NaIIonized aqueous solution
💧
⟶
AgI↓Ionized aqueous solution + NaNO3Ionized aqueous solution
Standard enthalpy
of reaction
ΔrH°
kJ · mol−1		Standard
Gibbs energy
of reaction
ΔrG°
kJ · mol−1		Standard entropy
of reaction
ΔrS°
J · K−1 · mol−1		Standard heat
capacity of reaction
at constant pressure
ΔrCp°
J · K−1 · mol−1
per 1 mol of
Equation
–−1.67––
per 1 mol of
–−1.67––
per 1 mol of
–−1.67––
per 1 mol of
–−1.67––
per 1 mol of
–−1.67––

Changes in aqueous solution (4)

Reaction of silver(I) nitrate and sodium iodide
◆
ΔrG−39.3 kJ/mol
K7.67 × 106
pK−6.89
AgNO3Un-ionized aqueous solution + NaIIonized aqueous solution
💧
⟶
AgI↓Un-ionized aqueous solution + NaNO3Ionized aqueous solution
Standard enthalpy
of reaction
ΔrH°
kJ · mol−1		Standard
Gibbs energy
of reaction
ΔrG°
kJ · mol−1		Standard entropy
of reaction
ΔrS°
J · K−1 · mol−1		Standard heat
capacity of reaction
at constant pressure
ΔrCp°
J · K−1 · mol−1
per 1 mol of
Equation
–−39.3––
per 1 mol of
–−39.3––
per 1 mol of
–−39.3––
per 1 mol of
–−39.3––
per 1 mol of
–−39.3––

Thermodynamic data of reactants

Chemical formulaStandard enthalpy
of formation
ΔfH°
kJ · mol−1		Standard Gibbs
energy of
formation
ΔfG°
kJ · mol−1		Standard
molar entropy
S°
J · K−1 · mol−1		Standard molar
heat capacity at
constant pressure
Cp°
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]––
NaI (cr)-287.78[1]-286.06[1]98.53[1]52.09[1]
NaI (g)-79.5[1]-121.0[1]248.978[1]36.65[1]
NaI (ai)-295.31[1]-313.47[1]170.3[1]-95.8[1]
NaI (cr)
1 hydrate
-883.096[1]-771.10[1]196.2[1]–
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution, (g):Gas

Thermodynamic data of products

Chemical formulaStandard enthalpy
of formation
ΔfH°
kJ · mol−1		Standard Gibbs
energy of
formation
ΔfG°
kJ · mol−1		Standard
molar entropy
S°
J · K−1 · mol−1		Standard molar
heat capacity at
constant pressure
Cp°
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]––
NaNO3 (cr)-467.85[1]-367.00[1]116.52[1]92.88[1]
NaNO3 (ai)-447.48[1]-373.15[1]205.4[1]-40.2[1]
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution

References

List of references

  1. 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
    National Institute of Standards and Technology (NIST)