Difference between revisions of "Potassium bismuthate"
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: Bi<sub>2</sub>O<sub>3</sub> + 6 KOH + 2 Cl<sub>2</sub> → 2 KBiO<sub>3</sub> + 4 KCl + 3 H<sub>2</sub>O | : Bi<sub>2</sub>O<sub>3</sub> + 6 KOH + 2 Cl<sub>2</sub> → 2 KBiO<sub>3</sub> + 4 KCl + 3 H<sub>2</sub>O | ||
| − | Fusing potassium superoxide and bismuth trioxide at high temperatures and pressure will yield potassium bismuthate.<ref>Baranov; Kim; Kim; Kang; Park; Pshirkov; Antipov; Physica. C, Superconductivity; vol. 357-360; nb. SUPPL. 2; (2001); p. 414 - 417</ref> | + | Fusing [[potassium superoxide]] and bismuth trioxide at high temperatures and pressure will yield potassium bismuthate.<ref>Baranov; Kim; Kim; Kang; Park; Pshirkov; Antipov; Physica. C, Superconductivity; vol. 357-360; nb. SUPPL. 2; (2001); p. 414 - 417</ref> |
: 2 KO<sub>2</sub> + Bi<sub>2</sub>O<sub>3</sub> → 2 KBiO<sub>3</sub> + ½ O<sub>2</sub> | : 2 KO<sub>2</sub> + Bi<sub>2</sub>O<sub>3</sub> → 2 KBiO<sub>3</sub> + ½ O<sub>2</sub> | ||
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Stirring a mixture of [[sodium bismuthate]] with potassium hydroxide for 6 hours at 250 °C will produce KBiO<sub>3</sub>.<ref>Saiduzzaman, Md; Yoshida, Hikaru; Takei, Takahiro; Yanagida, Sayaka; Kumada, Nobuhiro; Nagao, Masanori; Yamane, Hisanori; Azuma, Masaki; Rubel, Mirza H. K.; Moriyoshi, Chikako; Kuroiwa, Yoshihiro; Inorganic Chemistry; vol. 58; nb. 18; (2019); p. 11997 - 12001</ref> | Stirring a mixture of [[sodium bismuthate]] with potassium hydroxide for 6 hours at 250 °C will produce KBiO<sub>3</sub>.<ref>Saiduzzaman, Md; Yoshida, Hikaru; Takei, Takahiro; Yanagida, Sayaka; Kumada, Nobuhiro; Nagao, Masanori; Yamane, Hisanori; Azuma, Masaki; Rubel, Mirza H. K.; Moriyoshi, Chikako; Kuroiwa, Yoshihiro; Inorganic Chemistry; vol. 58; nb. 18; (2019); p. 11997 - 12001</ref> | ||
| − | The recommended literature preparation for potassium bismuthate is the oxidation of bismuth(III) oxide with a large excess of bromine in boiling 50% potassium hydroxide. The violet solid is suspended in water and decanted, during which time the color changes to red. The solid is dried over sulfuric acid and has the composition of KBiO<sub>3</sub> x 1/3 H<sub>2</sub>O.<ref>Scholder, R. and Stobbe, H., ''Z. Anorg. Allg. Chem.'' '''1941''', 247: 392-414. | + | The recommended literature preparation for potassium bismuthate is the oxidation of [[Bismuth trioxide|bismuth(III) oxide]] with a large excess of [[bromine]] in boiling 50% [[potassium hydroxide]]. The violet solid is suspended in water and decanted, during which time the color changes to red. The solid is dried over [[sulfuric acid]] and has the composition of KBiO<sub>3</sub> x 1/3 H<sub>2</sub>O.<ref>Scholder, R. and Stobbe, H., ''Z. Anorg. Allg. Chem.'' '''1941''', 247: 392-414. https://doi.org/10.1002/zaac.19412470404. For an english translation of this preparation see G. Brauer, ''Handbook of preparative inorganic chemistry'', Second edition '''1963''', p. 628-629</ref> |
==Projects== | ==Projects== | ||
Latest revision as of 22:02, 29 December 2021
| Names | |
|---|---|
| IUPAC name
Potassium bismuthate
| |
| Other names
Potassium bismuth oxide
Potassium bismuth trioxide | |
| Properties | |
| KBiO3 | |
| Molar mass | 296.077 g/mol |
| Appearance | Reddish or brown-reddish powdered solid |
| Odor | Odorless |
| Vapor pressure | ~0 mmHg |
| Thermochemistry | |
| Std enthalpy of
formation (ΔfH |
-683 kJ/mol[1] |
| Hazards | |
| Flash point | Non-flammable |
| Related compounds | |
| Related compounds
|
Sodium bismuthate |
| Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
| Infobox references | |
Potassium bismuthate is an inorganic chemical compound, a strong oxidizer with chemical formula KBiO3.
Like its sodium counterpart, potassium bismuthate is contaminated with side products from the synthesis as well as decomposition.
Contents
Properties
Chemical
Potassium bismuthate reacts with haloacids to will release their respective halogens. For example, reaction with hydrochloric acid will produce chlorine gas:
- KBiO3 + 6 HCl → KCl + BiCl3 + Cl2
This reaction is similar to the reaction between potassium permanganate with HCl.
Addition of hydrogen peroxide will cause it to decompose and release oxygen.
Physical
Potassium bismuthate is a reddish or brown-reddish solid, insoluble in cold water and decomposes in hot water.
Availability
Potassium bismuthate is sold by some chemical suppliers, albeit it's less available than sodium bismuthate. Usually the product is ~90% pure.[2]
Preparation
Can be prepared by bubbling chlorine gas through a hot suspension of potassium hydroxide and bismuth trioxide.[3]
- Bi2O3 + 6 KOH + 2 Cl2 → 2 KBiO3 + 4 KCl + 3 H2O
Fusing potassium superoxide and bismuth trioxide at high temperatures and pressure will yield potassium bismuthate.[4]
- 2 KO2 + Bi2O3 → 2 KBiO3 + ½ O2
Potassium oxide can also be used.[5]
Stirring a mixture of sodium bismuthate with potassium hydroxide for 6 hours at 250 °C will produce KBiO3.[6]
The recommended literature preparation for potassium bismuthate is the oxidation of bismuth(III) oxide with a large excess of bromine in boiling 50% potassium hydroxide. The violet solid is suspended in water and decanted, during which time the color changes to red. The solid is dried over sulfuric acid and has the composition of KBiO3 x 1/3 H2O.[7]
Projects
- Oxidizing agent
- Make permangante
- Compound collecting
Handling
Safety
Potassium bismuthate is an irritant if inhaled. Continued absorption of KBiO3 into body causes permanent kidney damage.
Storage
In closed plastic or glass bottles, away from moisture and acids.
Disposal
Can be neutralized by exposure to hot water or hydrogen peroxide and the bismuth recycled.
References
- ↑ Kasenov; Zhambekov; Kasenova; Russian Journal of Physical Chemistry; vol. 71; nb. 6; (1997); p. 1024 - 1026
- ↑ https://mateck.com/potassium-bismuthate.html
- ↑ Deichler, C.; Zeitschrift fur anorganische Chemie; vol. 20; (1899); p. 98-102
- ↑ Baranov; Kim; Kim; Kang; Park; Pshirkov; Antipov; Physica. C, Superconductivity; vol. 357-360; nb. SUPPL. 2; (2001); p. 414 - 417
- ↑ Khasanova; Yoshida; Yamamoto; Tajima; Physica. C, Superconductivity; vol. 356; nb. 1-2; (2001); p. 12 - 22
- ↑ Saiduzzaman, Md; Yoshida, Hikaru; Takei, Takahiro; Yanagida, Sayaka; Kumada, Nobuhiro; Nagao, Masanori; Yamane, Hisanori; Azuma, Masaki; Rubel, Mirza H. K.; Moriyoshi, Chikako; Kuroiwa, Yoshihiro; Inorganic Chemistry; vol. 58; nb. 18; (2019); p. 11997 - 12001
- ↑ Scholder, R. and Stobbe, H., Z. Anorg. Allg. Chem. 1941, 247: 392-414. https://doi.org/10.1002/zaac.19412470404. For an english translation of this preparation see G. Brauer, Handbook of preparative inorganic chemistry, Second edition 1963, p. 628-629
