Sodium Dithionite
Structure
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 dithionite ion has C2 geometry, almost eclipsed with a 16 O-S-S-O torsional angle. In the dihydrated form (Na2S2O4.2H2O), the dithionite anion has a shorter S-S bond length and a gauche 56 O-S-S-O torsional angle.
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. Reaction with formaldehyde produces Rongalite, which is used as a bleach, in, for instance, paper pulp, cotton, wool, Leather, Chrome Tanning agent and kaolin clay.
Na2S2O4 + 2 CH2O 2 HOCH2SO2 + 2 Na+
Sodium dithionite 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). 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
Dithionite
References
^ Pratt, L. A. (1924). "The Manufacture of Sodium Hyposulfite". Industrial & Engineering Chemistry 16: 676677. doi:10.1021/ie50175a006. edit
^ Weinrach, J. B. (1992). "A structural study of sodium dithionite and its ephemeral dihydrate: A new conformation for the dithionite ion". Journal of Crystallographic and Spectroscopic Research 22: 291301. doi:10.1007/BF01199531. edit
^ Herman Harry Szmant (1989). Organic building blocks of the chemical industry. John Wiley and Sons. p.113. ISBN 0471855456.
^ S.G. Mayhew. Eur. J. Biochem. 85, 535-547 (1978)
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Sodium compounds
NaAlO2 NaBH3(CN) NaBH4 NaBr NaBrO4 NaCH3COO NaCN NaC6H5CO2 NaC6H4(OH)CO2 NaCl NaClO NaClO2 NaClO3 NaClO4 NaF NaH NaHCO3 NaHSO3 NaHSO4 NaI NaIO3 NaIO4 NaMnO4 NaNH2 NaNO2 NaNO3 NaN3 NaOH NaO2 NaPO2H2 NaReO4 NaSCN NaSH NaTcO4 NaVO3 Na2CO3 Na2C2O4 Na2CrO4 Na2Cr2O7 Na2MnO4 Na2MoO4 Na2O Na2O2 Na2O(UO3)2 Na2S Na2SO3 Na2SO4 Na2S2O3 Na2S2O4 Na2S2O5 Na2S2O6 Na2S2O7 Na2S2O8 Na2SeO3 Na2SeO4 Na2SiO3 Na2Te Na2TeO3 Na2Ti3O7 Na2U2O7 NaWO4 Na2Zn(OH)4 Na3N Na3P Na3VO4 Na4Fe(CN)6 Na5P3O10
Categories: Bleaches | Dithionites | Sodium compoundsHidden categories: Chemboxes which contain changes to watched fields
Sodium Dithionite
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