Difference between revisions of "Silver perchlorate"
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==Properties== | ==Properties== | ||
===Chemical=== | ===Chemical=== | ||
| − | Silver perchlorate decomposes when heated to high temperatures, | + | Silver perchlorate decomposes when heated to high temperatures, releasing oxygen. |
| + | |||
| + | Silver perchlorate reacts with [[iodine]] to form [[silver iodide]] and iodine perchlorate. It was hypothesized originally that this reaction would yield chlorine tetraoxide, but later experiments proved that iodine perchlorate is formed instead:<ref>https://pubs.rsc.org/en/content/articlelanding/1962/JR/jr9620002510</ref> | ||
| + | |||
| + | : AgClO<sub>4</sub> + I<sub>2</sub> → AgI + IClO<sub>4</sub> | ||
===Physical=== | ===Physical=== | ||
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<references/> | <references/> | ||
===Relevant Sciencemadness threads=== | ===Relevant Sciencemadness threads=== | ||
| + | *[http://www.sciencemadness.org/talk/viewthread.php?tid=141289 Silver perchlorate incompatibilities] | ||
*[http://www.sciencemadness.org/talk/viewthread.php?tid=1576 ClO4 !?] | *[http://www.sciencemadness.org/talk/viewthread.php?tid=1576 ClO4 !?] | ||
*[http://www.sciencemadness.org/talk/viewthread.php?tid=9807 Perchlorate chemistry] | *[http://www.sciencemadness.org/talk/viewthread.php?tid=9807 Perchlorate chemistry] | ||
Latest revision as of 20:27, 21 October 2022
| Names | |
|---|---|
| IUPAC name
Silver perchlorate
| |
| Other names
Perchloric acid, silver(1+) salt
Silverperchlorate | |
| Properties | |
| AgClO4 | |
| Molar mass | 207.319 g/mol |
| Appearance | White solid |
| Density | 2.806 g/cm3 |
| Melting point | 486 °C (907 °F; 759 K) (decomposition) |
| Boiling point | Decomposes |
| 557 g/100 ml (25 °C) 792.8 g/100 ml (99 °C) | |
| Solubility | Soluble in alcohols |
| Vapor pressure | ~0 mmHg |
| Hazards | |
| Safety data sheet | Sigma-Aldrich |
| Related compounds | |
| Related compounds
|
Silver nitrate Silver sulfate |
| Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
| Infobox references | |
Silver perchlorate is a chemical compound with the formula AgClO4. It is a useful source of the Ag+ ions, due to its great solubility.
Contents
Properties
Chemical
Silver perchlorate decomposes when heated to high temperatures, releasing oxygen.
Silver perchlorate reacts with iodine to form silver iodide and iodine perchlorate. It was hypothesized originally that this reaction would yield chlorine tetraoxide, but later experiments proved that iodine perchlorate is formed instead:[1]
- AgClO4 + I2 → AgI + IClO4
Physical
Silver perchlorate is a white solid, very soluble in water. It is hygroscopic and tends to be commonly encountered as monohydrate.
Availability
Silver perchlorate is sometimes sold by chemical suppliers.
Preparation
Silver perchlorate can be made by dissolving silver metal in perchloric acid. Concentrate the resulting solution and cool it to recrystallize.
Projects
- Catalyst in organic reactions
- Make iodine perchlorate
- Flash powders
Handling
Safety
Silver perchlorate is a strong oxidizer and should be handled with care.
Being a soluble silver salt, ingestion is harmful.
Storage
In closed bottles, away from moisture and flammable materials.
Disposal
Silver perchlorate can be neutralized by reducing it with metallic iron. It can also be reduced to elemental silver with many common metals, like iron, zinc. The resulting silver metal should be recycled as it is expensive.
