This article relies largely or entirely on a
single source. (June 2013) |
Names | |
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IUPAC name
Silver(I) iodate
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Systematic IUPAC name
Silver(I) iodate(V) | |
Other names
Argentous iodate
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Identifiers | |
3D model (
JSmol)
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ChemSpider | |
ECHA InfoCard | 100.029.126 |
EC Number |
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PubChem
CID
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UNII | |
CompTox Dashboard (
EPA)
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Properties | |
AgIO3 | |
Molar mass | 282.77 g/mol |
Appearance | white crystals |
Odor | odorless |
Density | 5.525 g/cm3 |
Melting point | ~200 °C |
Boiling point | ~1150 °C |
0.003 g/100 mL (10 °C) 0.019 g/100 mL (50 °C) | |
Solubility product (Ksp)
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3.17×10−8 [1] |
Solubility | soluble in ammonia |
Structure | |
orthorhombic | |
Hazards | |
NFPA 704 (fire diamond) | |
Flash point | Non-combustable |
Related compounds | |
Other
anions
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silver iodide silver chlorate |
Other
cations
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sodium iodate potassium iodate |
Except where otherwise noted, data are given for materials in their
standard state (at 25 °C [77 °F], 100 kPa).
|
Silver iodate (AgIO3) is a light-sensitive, white crystal composed of silver, iodine and oxygen. Unlike most metal iodates, it is practically insoluble in water.
Silver iodate can be obtained by reacting silver nitrate (AgNO3) with sodium iodate or potassium iodate. The by-product of the reaction is sodium nitrate. [2]
Alternatively, it can be created by the action of iodine in a solution of silver oxide.
Silver iodate is used to detect traces of chlorides in blood.[ citation needed]
Silver nitrate reacts with iodate to form the precipitate of silver iodate, and the precipitate is transferred to silver nitrate.