Iron(III) sulfate

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Iron(III) sulfate
Names
IUPAC name
Iron(III) sulfate
Other names
Ferric sulfate
Sulfuric acid, iron(3+) salt (3:2)
Properties
Fe2(SO4)3
Molar mass 399.88 g/mol (anhydrous)
489.96 g/mol (pentahydrate)
562.00 g/mol (nonahydrate)
Appearance Gray-white solid
Density 3.097 g/cm3 (anhydrous)
1.898 g/cm3 (pentahydrate)
Melting point 480 °C (896 °F; 753 K) (anhydrous)
175 °C (347 °F) (nonahydrate)
Boiling point Decomposes
Slightly soluble
Solubility Sparingly soluble in alcohol
Negligible in acetone, ethyl acetate
Insoluble in sulfuric acid, ammonia
Hazards
Safety data sheet Sigma-Aldrich (hydrated)
Flash point Non-flammable
Related compounds
Related compounds
Iron(II) sulfate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Infobox references

Iron(III) sulfate also known as ferric sulfate or vitriol of Mars/vitriol martial, is the chemical compound with the formula Fe2(SO4)3, an iron salt.

Properties

Chemical

Ferric sulfate is used in industry as a coagulant.

Physical

Ferric sulfate is a yellow, hygroscopic compound. It is soluble in water, poorly soluble in organic solvents such as acetone, ethanol or various acetates. It is insoluble in sulfuric acid. The anhydrous form melts at 480 °C.

Availability

Iron(III) sulfate is available from many chemical suppliers.

One such seller on Amazon sells 4.5 kg of ferric sulfate at 18.40 $.

Preparation

Iron(III) sulfate can be made by reacting sulfuric acid, with a hot solution of ferrous sulfate, and an oxidizing agent, such as hydrogen peroxide.

2 FeSO4 + H2SO4 + H2O2 → Fe2(SO4)3 + 2H2O

This method is similar to the one used for obtaining ferric chloride.

n.b. Hydrogen peroxide is also a reducing agent and will reduce Iron(III) to to Iron(II).

Projects

Handling

Safety

Ferric sulfate both solid and as solution is corrosive to tissue and metallic objects.

Storage

Ferric sulfate should be stored in a tightly closed container, in a cool, dry place.

Disposal

Ferric sulfate can be neutralized with slaked lime.

References

Relevant Sciencemadness threads