Manganese(II) sulfate

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Manganese(II) sulfate
Manganese(II) sulfate bottle sample.jpg
MnSO4 sample and its original bottle. The compound is more pinkish in person.
Names
IUPAC name
Manganese(II) sulfate
Systematic IUPAC name
Manganese(II) sulfate
Other names
Manganese sulfate
Identifiers
Jmol-3D images Image
Properties
MnSO4
Molar mass 151.001 g/mol (anhydrous)
169.02 g/mol (monohydrate)
223.07 g/mol (tetrahydrate)
277.11 g/mol (heptahydrate)
Appearance White solid (anhydrous)
Pink crystalline solid (hydrated)
Odor Odorless
Density 3.25 g/cm3 (anhydrous)
2.95 g/cm3 (monohydrate)
2.107 g/cm3 (tetrahydrate)
Melting point 710 °C (1,310 °F; 983 K) (anhydrous)
27 °C (80.6 °F; 300.15 K) (tetrahydrate)
Boiling point 850 °C (1,560 °F; 1,120 K) (anhydrous)
52 g/100 mL (5 °C)
70 g/100 mL (7 °C)
Solubility Soluble in ethanol, methanol
Insoluble in diethyl ether, toluene
Hazards
Safety data sheet DoGEE (monohydrate)
Flash point Non-flammable
Related compounds
Related compounds
Chromium(III) sulfate
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

Manganese(II) sulfate is the sulfate salt of manganese, with the formula MnSO4. Although the anhydrous salt is white, its hydrates are pinkish in color.

Properties

Chemical

Manganese(II) sulfate will precipitate as manganese hydroxide when mixed with a strong base, such as sodium hydroxide.

Physical

Manganese sulfate is a pinkish crystalline salt, soluble in water, as well as primary alcohols, though insoluble in aprotic solvents, such as benzene or diethyl ether. It is most often encountered as monohydrate form, though other hydrates, like tetrahydrate, pentahydrate, and heptahydrate also exist.

Availability

Manganese sulfate is sold by various chemical suppliers.

Preparation

There are a few ways to make manganese(II) sulfate.

One involves the direct reaction of sulfuric acid with manganese metal:

H2SO4 + Mn → MnSO4 + H2

This reaction however, does not work with manganese dioxide, which is more available that manganese metal. There are a few ways around though:

One way is to react manganese dioxide with oxalic acid and then react the resulting manganese oxalate/carbonate with sulfuric acid.

Another method involves bubbling sulfur dioxide through a suspension of manganese dioxide in water, and the filtering the solution.

MnO2 + SO2 → MnSO4

You can also dissolve manganese alloys in sulfuric acid, however the resulting manganese sulfate will be contaminated with iron sulfate as well as other sulfates.

Projects

  • Make very pure manganese dioxide (chemically or electrochemically)
  • Source of manganese ions

Handling

Safety

Long-term exposure to manganese dust or compounds will lead to manganese poisoning, also known as manganism.

Storage

Manganese sulfate should be kept in closed plastic or glass bottles.

Disposal

Manganese sulfate should be precipitated to manganese dioxide and then sent to waste disposal centers. Waste batteries centers might also pick up manganese waste.

References

Relevant Sciencemadness threads