Ammonium bisulfate

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Ammonium bisulfate
Ammonium.svg Hydrogen sulfate.svg
Ball-and-stick model of an ammonium cation (left) and a bisulfite anion (right)
Sample of ammonium bisulfate.jpg
Identifiers
CAS number 7803-63-6 YesY
PubChem 16211166
ChemSpider 23057 YesY
RTECS number WS990000
Jmol-3D images Image 1
Properties
Molecular formula (NH4)HSO4
Molar mass 115.11 g/mol
Appearance White solid
Density 1.78 g/cm3
Melting point 147 °C (297 °F; 420 K)
Solubility in water Very soluble
Solubility in other solvents Soluble in methanol
insoluble in acetone
Hazards
MSDS External MSDS
EU Index Not listed
NFPA 704
Flammability code 0: Will not burn. E.g., water Health code 3: Short exposure could cause serious temporary or residual injury. E.g., chlorine gas Reactivity code 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g., liquid nitrogen Special hazards (white): no codeNFPA 704 four-colored diamond
Related compounds
Other anions Ammonium thiosulfate
Ammonium sulfite
Ammonium sulfate
Ammonium persulfate
Other cations Sodium bisulfate
Potassium bisulfate
Except where noted otherwise, data are given for materials in their standard state (at 25 °C (77 °F), 100 kPa)
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Infobox references

Ammonium bisulfate, also known as ammonium hydrogen sulfate, is a white, crystalline solid with formula (NH4)HSO4. It is the product of the half-neutralization of sulfuric acid by ammonia.

Production[edit]

It is commonly collected as a byproduct of the "acetone cyanohydrin route" to the commodity chemical methyl methacrylate.[1]

It can also be obtained by hydrolysis of sulfamic acid in aqueous solution, which produces the salt in high purity:

H3NSO3 + H2O → [NH4]+[HSO4]

It also arises by the thermal decomposition of ammonium sulfate:

(NH4)2SO4 → (NH4)HSO4 + NH3

Applications[edit]

It can be further neutralized with ammonia to form ammonium sulfate, a valuable fertilizer. It can be used as a weaker alternative to sulfuric acid, although sodium bisulfate is much more common.

References[edit]

  1. ^ William Bauer, Jr. "Methacrylic Acid and Derivatives" in Ullmann's Encyclopedia of Industrial Chemistry 2002, Wiley-VCH, Weinheim. doi:10.1002/14356007.a16_441.