Sodium dithionite: Difference between revisions
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:2 NaHSO<sub>3</sub> + Zn → Na<sub>2</sub>S<sub>2</sub>O<sub>4</sub> + Zn(OH)<sub>2</sub> |
:2 NaHSO<sub>3</sub> + Zn → Na<sub>2</sub>S<sub>2</sub>O<sub>4</sub> + Zn(OH)<sub>2</sub> |
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==Structure== |
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[[Raman spectroscopy]] and single-crystal X-ray diffraction studies of sodium dithionite in the solid state reveals that it exists in different forms. In one [[anhydrous]] form, the dithionate ion has C{{su|b=2}} geometry, almost eclipsed with a 16° O-S-S-O torsional angle. In the [[Hydrate|dihydrated]] form ({{chem|Na|2|S|2|O|4|.2H|2|O}}), the dithionite anion has a shorter S-S bond length and a gauche 56° O-S-S-O torsional angle.<ref>{{cite doi|10.1007/BF01199531}}</ref> |
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==Applications== |
==Applications== |
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Revision as of 18:01, 19 June 2009
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| Names | |
|---|---|
| Other names
D-Ox
Hydrolin Reductone Sodium hydrosulfite Sodium sulfoxylate Sulfoxylate Vatrolite Virtex L | |
| Identifiers | |
| ECHA InfoCard | 100.028.991 |
| EC Number |
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PubChem CID
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| RTECS number |
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CompTox Dashboard (EPA)
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| Properties | |
| Na2S2O4 | |
| Molar mass | 174.107 g/mol |
| Appearance | white to grayish crystalline powder |
| Density | 2.19 g/cm3, solid |
| Melting point | 52 °C (325 K) |
| Boiling point | Decomposes |
| very soluble | |
| Hazards | |
| NFPA 704 (fire diamond) | |
| Flash point | 100 °C |
| Related compounds | |
Other anions
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Sodium sulfite Sodium sulfate |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Sodium dithionite (also known as sodium hydrosulfite) is a white crystalline powder with a weak sulfurous odor. Although it is stable under most conditions, it will decompose in hot water and in acid solutions. It can be obtained from sodium bisulfite by the following reaction:
- 2 NaHSO3 + Zn → Na2S2O4 + Zn(OH)2
Structure
Raman spectroscopy and single-crystal X-ray diffraction studies of sodium dithionite in the solid state reveals that it exists in different forms. In one anhydrous form, the dithionate ion has C
2 geometry, almost eclipsed with a 16° O-S-S-O torsional angle. In the dihydrated form (Na
2S
2O
4.2H
2O), the dithionite anion has a shorter S-S bond length and a gauche 56° O-S-S-O torsional angle.[1]
Applications
Industry
This compound is a water-soluble salt, and can be used as a reducing agent in aqueous solutions. It is used as such in some industrial dying processes, where an otherwise water-insoluble dye can be reduced into a water-soluble alkali metal salt. The reduction properties of sodium dithionite also eliminate excess dye, residual oxide, and unintended pigments, thereby improving overall colour quality. It can also be used as a bleach, in, for instance, paper pulp, cotton, wool, and kaolin clay.
This chemical can also be used for water treatment, gas purification, cleaning, and stripping. It can also be used in industrial processes as a sulfonating agent or a sodium ion source. In addition to the textile industry, this compound is used in industries concerned with leather, foods, polymers, photography, and many others. Its wide use is attributable to its low toxicity LD 50 at 5 g/kg, and hence its wide range of applications.
Biological sciences
Sodium dithionite is often used in physiology experiments as a means of lowering solutions' redox potential (Eo' -0.66 V vs NHE at pH 7[2]). Potassium ferricyanide is usually used as an oxidizing chemical in such experiments (Eo' ~ 436 mV at pH 7). In addition, sodium dithionite is often used in soil chemistry experiments to determine the amount of iron that is not incorporated in primary silicate minerals. Hence, iron extracted by sodium dithionite is also referred to as "free iron." The strong affinity of the dithionite ion for bi- and trivalent metal cations (M2+, M3+) allows it to enhance the solubility of iron, and therefore dithionite is a useful chelating agent. When you heat the reaction, rainbow colors emerge due to the high transition states of energy.
Geosciences
Sodium dithionite has been used in chemical Enhanced Oil Recovery to stabilize polyacrylamide polymers against radical degradation in the presence of iron. It has also been used in environmental applications to propagate a low Eh front in the subsurface in order to reduce pollutants such as chromium.
See also
References
- ^ Attention: This template ({{cite doi}}) is deprecated. To cite the publication identified by doi:10.1007/BF01199531, please use {{cite journal}} (if it was published in a bona fide academic journal, otherwise {{cite report}} with
|doi=10.1007/BF01199531instead. - ^ S.G. Mayhew. Eur. J. Biochem. 85, 535-547 (1978)