Difference between revisions of "Iron(III) sulfate"
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Iron(III) sulfate can be made by reacting [[sulfuric acid]], with a hot solution of [[Iron(II) sulfate|ferrous sulfate]], and an oxidizing agent, such as [[hydrogen peroxide]]. | Iron(III) sulfate can be made by reacting [[sulfuric acid]], with a hot solution of [[Iron(II) sulfate|ferrous sulfate]], and an oxidizing agent, such as [[hydrogen peroxide]]. | ||
| − | : | + | :2 FeSO<sub>4</sub> + H<sub>2</sub>SO<sub>4</sub> + H<sub>2</sub>O<sub>2</sub> → Fe<sub>2</sub>(SO<sub>4</sub>)<sub>3</sub> + 2H<sub>2</sub>O |
| + | |||
| + | This method is similar to the one used for obtaining [[iron(III) chloride|ferric chloride]]. | ||
==Projects== | ==Projects== | ||
Revision as of 19:17, 18 November 2015
Iron(III) sulfate also known as ferric sulfate, is the chemical compound with the formula Fe2(SO4)3.
Contents
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.
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.
