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2AgNO3 + MgCl2 💧→ 2AgCl↓ + Mg(NO3)2

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Reaction of silver(I) nitrate and magnesium chloride
2AgNO3Silver(I) nitrate + MgCl2Magnesium chloride
💧
⟶
2AgCl↓Silver(I) chloride + Mg(NO3)2Magnesium nitrate

The reaction of silver(I) nitrate and magnesium chloride yields silver(I) chloride and magnesium 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 magnesium chloride
2AgNO3Silver(I) nitrate + MgCl2Magnesium chloride
💧
⟶
2AgCl↓Silver(I) chloride + Mg(NO3)2Magnesium 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 magnesium chloride

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
AgNO3Silver(I) nitrate2
Lewis acid
Very soluble in water
MgCl2Magnesium chloride1
Lewis base
Very soluble in water

Products

Chemical formulaNameCoefficientTypeType in general
equation
AgClSilver(I) chloride2
Lewis conjugate
Insoluble in water
Mg(NO3)2Magnesium nitrate1
Non-redox product
–

Thermodynamic changes

Changes in standard condition

Reaction of silver(I) nitrate and magnesium chloride
◆
ΔrG−150.4 kJ/mol
K2.23 × 1026
pK−26.35
2AgNO3Crystalline solid + MgCl2Crystalline solid
💧
⟶
2AgCl↓Crystalline solid + Mg(NO3)2Crystalline 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
−154.69−150.4−15.1−13.98
per 1 mol of
−77.345−75.20−7.55−6.990
per 1 mol of
−154.69−150.4−15.1−13.98
per 1 mol of
−77.345−75.20−7.55−6.990
per 1 mol of
−154.69−150.4−15.1−13.98

Changes in aqueous solution (1)

Reaction of silver(I) nitrate and magnesium chloride
◆
ΔrG−0.1 kJ/mol
K1.04 × 100
pK−0.02
2AgNO3Ionized aqueous solution + MgCl2Ionized aqueous solution
💧
⟶
2AgCl↓Ionized aqueous solution + Mg(NO3)2Ionized 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
0.02−0.10.1–
per 1 mol of
0.0100−0.0500.050–
per 1 mol of
0.0200−0.100.10–
per 1 mol of
0.0100−0.0500.050–
per 1 mol of
0.0200−0.100.10–

Changes in aqueous solution (2)

Reaction of silver(I) nitrate and magnesium chloride
◆
ΔrG−37.5 kJ/mol
K3.71 × 106
pK−6.57
2AgNO3Ionized aqueous solution + MgCl2Ionized aqueous solution
💧
⟶
2AgCl↓Un-ionized aqueous solution + Mg(NO3)2Ionized 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
−22.4−37.549.5–
per 1 mol of
−11.2−18.824.8–
per 1 mol of
−22.4−37.549.5–
per 1 mol of
−11.2−18.824.8–
per 1 mol of
−22.4−37.549.5–

Changes in aqueous solution (3)

Reaction of silver(I) nitrate and magnesium chloride
◆
ΔrG−3.5 kJ/mol
K4.10 × 100
pK−0.61
2AgNO3Un-ionized aqueous solution + MgCl2Ionized aqueous solution
💧
⟶
2AgCl↓Ionized aqueous solution + Mg(NO3)2Ionized 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
–−3.5––
per 1 mol of
–−1.8––
per 1 mol of
–−3.5––
per 1 mol of
–−1.8––
per 1 mol of
–−3.5––

Changes in aqueous solution (4)

Reaction of silver(I) nitrate and magnesium chloride
◆
ΔrG−40.8 kJ/mol
K1.41 × 107
pK−7.15
2AgNO3Un-ionized aqueous solution + MgCl2Ionized aqueous solution
💧
⟶
2AgCl↓Un-ionized aqueous solution + Mg(NO3)2Ionized 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
–−40.8––
per 1 mol of
–−20.4––
per 1 mol of
–−40.8––
per 1 mol of
–−20.4––
per 1 mol of
–−40.8––

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]––
MgCl2 (cr)-641.32[1]-591.79[1]89.62[1]71.38[1]
MgCl2 (g)-400.4[1]–––
MgCl2 (ai)-801.15[1]-717.1[1]-25.1[1]–
MgCl2 (cr)
1 hydrate
-966.63[1]-861.74[1]137.2[1]115.27[1]
MgCl2 (cr)
2 hydrate
-1279.72[1]-1118.00[1]179.9[1]159.20[1]
MgCl2 (cr)
4 hydrate
-1898.99[1]-1623.29[1]264.0[1]241.42[1]
MgCl2 (cr)
6 hydrate
-2499.02[1]-2114.64[1]366.1[1]315.06[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
AgCl (cr)-127.068[1]-109.789[1]96.2[1]50.79[1]
AgCl (g)––245.92[1]35.86[1]
AgCl (ai)-61.580[1]-54.120[1]129.3[1]-114.6[1]
AgCl (ao)-72.8[1]-72.8[1]154.0[1]–
Mg(NO3)2 (cr)-790.65[1]-589.4[1]164.0[1]141.92[1]
Mg(NO3)2 (ai)-881.57[1]-677.3[1]154.8[1]–
Mg(NO3)2 (cr)
2 hydrate
-1409.2[1]–––
Mg(NO3)2 (cr)
6 hydrate
-2613.28[1]-2080.3[1]452[1]–
* (cr):Crystalline solid, (g):Gas, (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)