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Silver permanganate

From Wikipedia, the free encyclopedia

Silver permanganate
Names
IUPAC name
Silver(I) permanganate
Systematic IUPAC name
Silver(I) manganate(VII)
Other names
Argentous permanganate
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.029.127 Edit this at Wikidata
EC Number
  • 232-040-1
UNII
  • InChI=1S/Ag.Mn.4O/q+1;;;;;-1
    Key: FBDQITNNUANGAD-UHFFFAOYSA-N
  • InChI=1/Ag.Mn.4O/q+1;;;;;-1/rAg.MnO4/c;2-1(3,4)5/q+1;-1
    Key: FBDQITNNUANGAD-URBVJNAFAD
  • [Ag+].[O-][Mn](=O)(=O)=O
Properties
AgMnO4
Molar mass 226.804 g/mol
Appearance purple crystals or gray powder
Density 4.27 g/cm3
Melting point 160 °C (320 °F; 433 K) (decomposes)
0.55 g/100 mL (0 °C)
1.69 g/100 mL (30 °C)
−63.0·10−6 cm3/mol
Structure
monoclinic
Hazards
Occupational safety and health (OHS/OSH):
Main hazards
 Eye irritant
GHS labelling:
GHS03: Oxidizing
GHS07: Exclamation mark
Warning
H272, H312, H319, H332
P210, P220, P261, P264, P270, P271, P280, P301+P310, P302+P352, P304+P340, P305+P351+P338, P311, P321, P330, P337+P313, P362+P364, P370+P378, P501
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

Silver permanganate is an inorganic compound with the chemical formula AgMnO4. This salt is a purple crystal adopting a monoclinic crystal system.[1] It decomposes when heated or mixed with water, and heating to high temperature may lead to explosion. The compound is used in gas masks.[citation needed]

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  • turning silver bars into a chemical christmas tree
  • penny vs. nitric acid
  • Chemical Chameleon Demonstration (with NaOH, KMnO4, and Sucrose)
  • Removing Silver Nitrate Stains
  • SLOW MOTION CHEMISTRY! Potassium Permanganate and Hydrogen Peroxide

Transcription

Production

It can be produced through the reaction of silver nitrate and potassium permanganate:[2]

AgNO3 + KMnO4 → AgMnO4 + KNO3

References

  1. ^ Boonstra, E. G. (14 August 1968). "The crystal structure of silver permanganate". Acta Crystallographica Section B. 24 (8): 1053–1062. Bibcode:1968AcCrB..24.1053B. doi:10.1107/S0567740868003699.
  2. ^ Greenwood, Norman  N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.


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This page was last edited on 1 April 2024, at 19:21
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