Sodium dithionite

Source: Wikipedia, the free encyclopedia.
"Sodium hydrosulfite" redirects here. For sodium hydrogen sulfite (NaHSO3), sometimes erroneously referred to as sodium hydrosulfite, see Sodium bisulfite.
Not to be confused with Sodium hydrosulfide or Sodium dithionate.
Sodium dithionite
Sodium dithionite
Names
Other names
D-Ox, Hydrolin, Reductone
sodium hydrosulfite, sodium sulfoxylate, Sulfoxylate
Vatrolite, Virtex L
Hydrosulfit, Prayon
Blankit, Albite A, Konite
Zepar, Burmol, Arostit
Identifiers
3D model (
JSmol
)
ChEBI
ChemSpider
ECHA InfoCard
 100.028.991 Edit this at Wikidata
EC Number
  • 231-890-0
RTECS number
  • JP2100000
UNII
UN number 1384
  • InChI=1S/2Na.H2O4S2/c;;1-5(2)6(3)4/h;;(H,1,2)(H,3,4)/q2*+1;/p-2
    Key: JVBXVOWTABLYPX-UHFFFAOYSA-L
  • [O-]S(=O)S(=O)[O-].[Na+].[Na+]
Properties
Na2S2O4
Molar mass 174.107 g/mol (anhydrous)
210.146 g/mol (dihydrate)
Appearance white to grayish crystalline powder
light-lemon colored flakes
Odor faint sulfur odor
Density 2.38 g/cm3 (anhydrous)
1.58 g/cm3 (dihydrate)
Melting point 52 °C (126 °F; 325 K)
Boiling point Decomposes
18.2 g/100 mL (anhydrous, 20 °C)
21.9 g/100 mL (Dihydrate, 20 °C)
Solubility slightly soluble in alcohol
Hazards
GHS labelling:
GHS02: FlammableGHS07: Exclamation mark
Danger
H251, H302
P235+P410, P264, P270, P280, P301+P312, P330, P407, P413, P420, P501
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 2: Intense or continued but not chronic exposure could cause temporary incapacitation or possible residual injury. E.g. chloroformFlammability 3: Liquids and solids that can be ignited under almost all ambient temperature conditions. Flash point between 23 and 38 °C (73 and 100 °F). E.g. gasolineInstability 1: Normally stable, but can become unstable at elevated temperatures and pressures. E.g. calciumSpecial hazards (white): no code
2
3
1
Flash point 100 °C (212 °F; 373 K)
200 °C (392 °F; 473 K)
Related compounds
Other anions
 Sodium sulfite
Sodium sulfate
Related compounds
 Sodium thiosulfate
Sodium bisulfite
Sodium metabisulfite
Sodium bisulfate
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 sulfurous odor. Although it is stable in dry air, it decomposes in hot water and in acid solutions.

Structure

The structure has been examined by

gauche 56° O-S-S-O torsional angle.[1]

A weak S-S bond is indicated by the S-S distance of 239 pm, which is elongated by ca. 30 pm relative to a typical S-S bond.

EPR spectroscopy. It is also observed that 35S undergoes rapid exchange between S2O42− and SO2 in neutral or acidic solution, consistent with the weak S-S bond in the anion.[3]

Preparation

Sodium dithionite is produced industrially by reduction of sulfur dioxide. Approximately 300,000 tons were produced in 1990.[4] The route using zinc powder is a two-step process:

2 SO2 + Zn → ZnS2O4
ZnS2O4 + 2 NaOH → Na2S2O4 + Zn(OH)2

The sodium borohydride method obeys the following stoichiometry:

NaBH4 + 8 NaOH + 8 SO2 → 4 Na2S2O4 + NaBO2 + 6 H2O

Each equivalent of H− reduces two equivalents of sulfur dioxide. Formate has also been used as the reductant.

Properties and reactions

Hydrolysis

Sodium dithionite is stable when dry, but aqueous solutions deteriorate due to the following reaction:

2 S2O42− + H2O → S2O32− + 2 HSO3−

This behavior is consistent with the instability of dithionous acid. Thus, solutions of sodium dithionite cannot be stored for a long period of time.[3]

Anhydrous sodium dithionite decomposes to sodium sulfate and sulfur dioxide above 90 °C in the air. In absence of air, it decomposes quickly above 150 °C to sodium sulfite, sodium thiosulfate, sulfur dioxide and trace amount of sulfur.

Redox reactions

Sodium dithionite is a reducing agent. At pH 7, the potential is -0.66 V compared to the normal hydrogen electrode. Redox occurs with formation of bisulfite:[5]

S2O42- + 2 H2O → 2 HSO3− + 2 e− + 2 H+

Sodium dithionite reacts with oxygen:

Na2S2O4 + O2 + H2O → NaHSO4 + NaHSO3

These reactions exhibit complex pH-dependent equilibria involving bisulfite, thiosulfate, and sulfur dioxide.

With organic carbonyls

In the presence of aldehydes, sodium dithionite reacts either to form α-hydroxy-sulfinates at room temperature or to reduce the aldehyde to the corresponding alcohol above a temperature of 85 °C.[6][7] Some ketones are also reduced under similar conditions.

Applications

Industry

Being water-soluble, sodium dithionite is used as a reducing agent in some industrial dyeing processes. In the case of sulfur dyes and vat dyes, an otherwise water-insoluble dye can be reduced into a water-soluble alkali metal salt (e.g. indigo dye).[8]

Sodium dithionite can also be used for water treatment, aquarium water conditioners, gas purification, cleaning, and stripping. It has also been applied as a sulfonating agent. In addition to the textile industry, this compound is used in industries concerned with leather, foods, polymers, photography, and many others, often as a decolourising agent. It is even used domestically as a decoloring agent for white laundry, when it has been accidentally stained by way of a dyed item slipping into the high temperature washing cycle. It is usually available in 5 gram sachets termed hydrosulfite after the antiquated name of the salt.

It is the active ingredient in "Iron Out Rust Stain Remover", a commercial rust product.[9]

Laboratory

Sodium dithionite is often used in

chelating agent
.

Aqueous solutions of sodium dithionite were once used to produce '

peracid followed by substitution using sodium dithionite to introduce the thiol functional group.[12]

Photography

It is used in Kodak fogging developer, FD-70. This is used in the second step in processing black and white positive images, for making slides. It is part of the Kodak Direct Positive Film Developing Outfit.[13]

Safety

The wide use of sodium dithionite is attributable in part to its low toxicity LD50 at 2.5 g/kg (rats, oral).[4]

See also

References

  1. S2CID 97124638
    .
  2. ISBN 978-0-08-037941-8
    .
  3. ^
    ISBN 978-0-13-175553-6
    .
  4. ^
    ISBN 978-3527306732
    .
  5. PMID 648533
    .
  6. ^ J. Org. Chem., 1980, 45 (21), pp 4126–4129, http://pubs.acs.org/doi/abs/10.1021/jo01309a011
  7. ^ "Aldehyde sulfoxylate systemic fungicides". google.com. Archived from the original on 27 April 2018. Retrieved 27 April 2018.
  8. doi:10.1016/j.dyepig.2006.05.041
    .
  9. ^ "The Best Rust Removers for Restoring Every Surface". 23 March 2023.
  10. PMID 648533
    .
  11. doi:10.1021/ed066p359.2
  12. ISBN 978-0471936237
    .
  13. ^ "Kodak Direct Positive Film 5246" (PDF). 125px.com. Kodak. Retrieved 6 November 2019.

External links

  • Sodium dithionite - ipcs inchem[1]
  1. ^ "Sodium dithionite - ipcs inchem" (PDF). www.inchem.org. Berliln, Germany. 2004. Archived from the original (PDF) on 17 April 2018. Retrieved 15 June 2018.
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