Difference between revisions of "Chlorite"
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Sodium chlorite can be made by reducing [[sodium chlorate]] in a strong acid solution with a suitable reducing agent, like [[sodium sulfite]], [[sulfur dioxide]] or even [[hydrochloric acid]]. This produces [[chlorine dioxide]], which is then absorbed into an alkaline solution and reduced with [[hydrogen peroxide]], yielding sodium chlorite. The final product will always contain 20% sodium chloride. | Sodium chlorite can be made by reducing [[sodium chlorate]] in a strong acid solution with a suitable reducing agent, like [[sodium sulfite]], [[sulfur dioxide]] or even [[hydrochloric acid]]. This produces [[chlorine dioxide]], which is then absorbed into an alkaline solution and reduced with [[hydrogen peroxide]], yielding sodium chlorite. The final product will always contain 20% sodium chloride. | ||
| − | Reaction of [[chlorine]] with [[sodium nitrate]] will yield sodium chlorite and [[nitrosyl chloride]]. | + | Reaction of [[chlorine]] with [[sodium nitrate]] will yield [[sodium chlorite]] and [[nitrosyl chloride]]. |
: NaNO<sub>3</sub> + Cl<sub>2</sub> → NaClO<sub>2</sub> + NOCl | : NaNO<sub>3</sub> + Cl<sub>2</sub> → NaClO<sub>2</sub> + NOCl | ||
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==Safety and handling== | ==Safety and handling== | ||
| − | Chlorites are powerful oxidizers. | + | Chlorites are powerful oxidizers. Avoid contact with acids, as the reaction will release toxic chlorine dioxide. |
==References== | ==References== | ||
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*[http://www.sciencemadness.org/talk/viewthread.php?tid=18929 Chlorite production] | *[http://www.sciencemadness.org/talk/viewthread.php?tid=18929 Chlorite production] | ||
| + | [[Category:Chemical compounds]] | ||
| + | [[Category:Inorganic compounds]] | ||
[[Category:Anions]] | [[Category:Anions]] | ||
[[Category:Oxoanions]] | [[Category:Oxoanions]] | ||
Latest revision as of 22:13, 16 September 2020
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A chlorite is a compound that contains the chlorite ion, ClO−
2.
Contents
General properties
Chlorite is the strongest oxidizer of the chlorine oxyanions, on the basis of standard half cell potentials.[1]
Chlorite salts, like sodium chlorite reacts with acids and elemental chlorine to yield chlorine dioxide.
- 2 NaClO2 + Cl2 → 2 ClO2 + 3 NaCl + H2O
- 5 NaClO2 + 4 HCl → 5 NaCl + 4 ClO2 + 2 H2O
The parental acid, chlorous acid is unstable and decomposes to hypochlorous and chloric acids
Salts like ammonium chlorite, are impossible to obtain, as the chlorous anion will oxidize the ammonium cation.
Availability
Chlorites, like sodium or potassium chlorite can be purchased from lab suppliers.
Preparation
Sodium chlorite can be made by reducing sodium chlorate in a strong acid solution with a suitable reducing agent, like sodium sulfite, sulfur dioxide or even hydrochloric acid. This produces chlorine dioxide, which is then absorbed into an alkaline solution and reduced with hydrogen peroxide, yielding sodium chlorite. The final product will always contain 20% sodium chloride.
Reaction of chlorine with sodium nitrate will yield sodium chlorite and nitrosyl chloride.
- NaNO3 + Cl2 → NaClO2 + NOCl
Similar techniques can be done for other chlorite salts.
Safety and handling
Chlorites are powerful oxidizers. Avoid contact with acids, as the reaction will release toxic chlorine dioxide.
References
- ↑ Cotton, F. Albert; Wilkinson, Geoffrey (1988), Advanced Inorganic Chemistry (5th ed.), New York: Wiley-Interscience, p. 564
