MnSO4 sample and its original bottle. The compound is more pinkish in person.
| IUPAC name
| Systematic IUPAC name
| Other names
|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)
|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
|Safety data sheet||DoGEE (monohydrate)|
| Chromium(III) sulfate|
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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.
Manganese(II) sulfate will precipitate as manganese hydroxide when mixed with a strong base, such as sodium hydroxide.
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.
Manganese sulfate is sold by various chemical suppliers.
There are a few ways to make manganese(II) sulfate.
- 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.
- Make very pure manganese dioxide (chemically or electrochemically)
- Source of manganese ions
Long-term exposure to manganese dust or compounds will lead to manganese poisoning, also known as manganism.
Manganese sulfate should be kept in closed plastic or glass bottles.
Manganese sulfate should be precipitated to manganese dioxide and then sent to waste disposal centers. Waste batteries centers might also pick up manganese waste.