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MgI2 + 2NH4F 💧→ MgF2↓ + 2NH4I

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Reaction of magnesium iodide and ammonium fluoride
MgI2Magnesium iodide + 2NH4FAmmonium fluoride
💧
⟶
MgF2↓Magnesium fluoride + 2NH4IAmmonium iodide

The reaction of magnesium iodide and ammonium fluoride yields magnesium fluoride and ammonium iodide. 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 magnesium iodide and ammonium fluoride
MgI2Magnesium iodide + 2NH4FAmmonium fluoride
💧
⟶
MgF2↓Magnesium fluoride + 2NH4IAmmonium iodide

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 magnesium iodide and ammonium fluoride

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
MgI2Magnesium iodide1
Lewis acid
Very soluble in water
NH4FAmmonium fluoride2
Lewis base
Very soluble in water

Products

Chemical formulaNameCoefficientTypeType in general
equation
MgF2Magnesium fluoride1
Lewis conjugate
Insoluble in water
NH4IAmmonium iodide2
Non-redox product
–

Thermodynamic changes

Changes in standard condition

Reaction of magnesium iodide and ammonium fluoride
◆
ΔrG−239.6 kJ/mol
K9.46 × 1041
pK−41.98
MgI2Crystalline solid + 2NH4FCrystalline solid
💧
⟶
MgF2↓Crystalline solid + 2NH4ICrystalline 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
−234.3−239.618–
per 1 mol of
−234.3−239.618–
per 1 mol of
−117.2−119.89.0–
per 1 mol of
−234.3−239.618–
per 1 mol of
−117.2−119.89.0–

Changes in aqueous solution

Reaction of magnesium iodide and ammonium fluoride
◆
ΔrG−57.7 kJ/mol
K1.28 × 1010
pK−10.11
MgI2Ionized aqueous solution + 2NH4FIonized aqueous solution
💧
⟶
MgF2↓Crystalline solid + 2NH4IIonized 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
8.7−57.7222.9–
per 1 mol of
8.7−57.7222.9–
per 1 mol of
4.3−28.9111.5–
per 1 mol of
8.7−57.7222.9–
per 1 mol of
4.3−28.9111.5–

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
MgI2 (cr)-364.0[1]-358.2[1]129.7[1]–
MgI2 (g)-172[1]–––
MgI2 (ai)-577.22[1]-558.1[1]84.5[1]–
NH4F (cr)-463.96[1]-348.68[1]71.96[1]65.27[1]
NH4F (ai)-465.14[1]-358.09[1]99.6[1]-26.8[1]
* (cr):Crystalline solid, (g):Gas, (ai):Ionized aqueous solution

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
MgF2 (cr)-1123.4[1]-1070.2[1]57.24[1]61.59[1]
MgF2 (g)-723.8[1]-730.5[1]258.39[1]48.62[1]
NH4I (cr)-201.42[1]-112.5[1]117[1]–
NH4I (ai)-187.69[1]-130.88[1]224.7[1]-62.3[1]
* (cr):Crystalline solid, (g):Gas, (ai):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)