Chemistry:Sodium thiosulfate
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| IUPAC name
Sodium thiosulfate
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| Other names
Sodium hyposulphite
Hyposulphite of soda Hypo | |
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3D model (JSmol)
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| Properties | |
| Na 2S 2O 3 | |
| Molar mass | 158.11 g/mol (anhydrous) 248.18 g/mol (pentahydrate) |
| Appearance | White crystals |
| Odor | Odorless |
| Density | 1.667 g/cm3 |
| Melting point | 48.3 °C (118.9 °F; 321.4 K) (pentahydrate) |
| Boiling point | 100 °C (212 °F; 373 K) (pentahydrate, - 5H2O decomposition) |
| 70.1 g/100 mL (20 °C)[1] 231 g/100 mL (100 °C) | |
| Solubility | negligible in alcohol |
Refractive index (nD)
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1.489 |
| Structure | |
| monoclinic | |
| Hazards | |
| Safety data sheet | External MSDS |
| GHS pictograms | 
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| GHS Signal word | Warning |
| H315, H319, H335 | |
| P261, P264, P271, P280, P302+352, P304+340, P305+351+338, P312, P321, P332+313, P337+313, P362, P403+233, P405, P501 | |
| NFPA 704 (fire diamond) | |
| Flash point | Non-flammable |
| Related compounds | |
Other cations
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Thiosulfuric acid Lithium thiosulfate Potassium thiosulfate |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
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| Infobox references | |
Sodium thiosulfate (sodium thiosulphate) is an inorganic compound with the formula Na
2S
2O
3 · (H
2O)(x) .Typically it is available as the white or colorless pentahydrate (x = 5), It is a white solid that dissolves well in water. The compound is a reducing agent and a ligand, and these properties underpin its applications.[2]
Uses
Sodium thiosulfate is used predominantly in dyeing. It converts some dyes to their soluble colorless "leuco" forms,. It is also used to bleach "wool, cotton, silk, ...soaps, glues, clay, sand, bauxite, and... edible oils, edible fats, and gelatin."[2]
Medical uses
Sodium thiosulfate is used in the treatment of cyanide poisoning.[3] It is on the World Health Organization's List of Essential Medicines.[4][5] Other uses include topical treatment of ringworm and tinea versicolor,[3][6] and treating some side effects of hemodialysis[7] and chemotherapy.[8][9] In September 2022, the U.S. Food and Drug Administration (FDA) approved sodium thiosulfate under the trade name Pedmark to lessen the risk of ototoxicity and hearing loss in infant, child, and adolescent cancer patients receiving the chemotherapy medication cisplatin.[10][11]
Photographic processing
In photography, sodium thiosulfate is known as a fixer and 'hypo', from the original chemical name, hyposulphite of soda.[12] It functions to dissolve silver halides, e.g., AgBr, components of photographic emulsions. It is used for both film and photographic paper processing. Ammonium thiosulfate is typically preferred to sodium thiosulfate for this application.[2] The ability of thiosulfate to dissolve silver ions is related to its ability to dissolve gold ions described below.
Neutralizing chlorinated water
It is used to dechlorinate tap water including lowering chlorine levels for use in aquariums, swimming pools, and spas (e.g., following superchlorination) and within water treatment plants to treat settled backwash water prior to release into rivers.[2] The reduction reaction is analogous to the iodine reduction reaction.
In pH testing of bleach substances, sodium thiosulfate neutralizes the color-removing effects of bleach and allows one to test the pH of bleach solutions with liquid indicators. The relevant reaction is akin to the iodine reaction: thiosulfate reduces the hypochlorite (the active ingredient in bleach) and in so doing becomes oxidized to sulfate. The complete reaction is:
- 4 NaClO + Na
2S
2O
3 + 2 NaOH → 4 NaCl + 2 Na
2SO
4 + H
2O
Similarly, sodium thiosulfate reacts with bromine, removing the free bromine from the solution. Solutions of sodium thiosulfate are commonly used as a precaution in chemistry laboratories when working with bromine and for the safe disposal of bromine, iodine, or other strong oxidizers.
Structure
Two polymorphs are known as pentahydrate. The anhydrous salt exists in several polymorphs.[2] In the solid state, the thiosulfate anion is tetrahedral in shape and is notionally derived by replacing one of the oxygen atoms by a sulfur atom in a sulfate anion. The S-S distance indicates a single bond, implying that the terminal sulfur holds a significant negative charge and the S-O interactions have more double-bond character.
Production
Sodium thiosulfate is prepared by oxidation of sodium sulfite with sulfur.[2] It is also produced from waste sodium sulfide from the manufacture of sulfur dyes.[13]
This salt can also be prepared by boiling aqueous sodium hydroxide and sulfur according to the following equation.[14][15] However, this is not recommended outside of a laboratory, as exposure to hydrogen sulfide can result if improperly handled.
- 6 NaOH + 4 S → 2 Na
2S + Na
2S
2O
3 + 3 H
2O
Principal reactions
Upon heating to 300 °C, it decomposes to sodium sulfate and sodium polysulfide:
- 4 Na
2S
2O
3 → 3 Na
2SO
4 + Na
2S
5
Thiosulfate salts characteristically decompose upon treatment with acids. Initial protonation occurs at sulfur. When the protonation is conducted in diethyl ether at −78 °C, H
2S
2O
3 (thiosulfuric acid) can be obtained. It is a somewhat strong acid with pKas of 0.6 and 1.7 for the first and second dissociations, respectively. Under normal conditions, acidification of solutions of this salt excess with even dilute acids results in complete decomposition to sulfur, sulfur dioxide, and water:[13]
- 8 Na
2S
2O
3 + 16 HCl → 16 NaCl + S
8 + 8 SO
2 + 8 H
2O
Coordination chemistry
Thiosulfate is a potent ligand for soft metal ions. A typical complex is [Pd(S
2O
3)
2(ethylenediamine)]2−, which features a pair of S-bonded thiosulfate ligands. Sodium thiosulfate and ammonium thiosulfate have been proposed as alternative lixiviants to cyanide for extraction of gold.[16][2] The advantages of this approach are that (i) thiosulfate is far less toxic than cyanide and (ii) that ore types that are refractory to gold cyanidation (e.g. carbonaceous or Carlin-type ores) can be leached by thiosulfate. Some problems with this alternative process include the high consumption of thiosulfate, and the lack of a suitable recovery technique, since [Au(S
2O
3)
2]3− does not adsorb to activated carbon, which is the standard technique used in gold cyanidation to separate the gold complex from the ore slurry. However, an electrolytic process for recovering Au with divalent copper has been developed.[17]
Iodometry
Some analytical|procedures exploit the oxidizability of thiosulfate anion by iodine. The reaction produces tetrathionate:
- 2 S
2O2−
3 + I
2 → S
4O2−
6 + 2 I−
Due to the quantitative nature of this reaction, as well as because Na
2S
2O
3 · 5H2O has an excellent shelf-life, it is used as a titrant in iodometry. Na
2S
2O
3 · 5H2O is also a component of iodine clock experiments.
This particular use can be set up to measure the oxygen content of water through a long series of reactions in the Winkler test for dissolved oxygen. It is also used in estimating volumetrically the concentrations of certain compounds in solution (hydrogen peroxide, for instance) and in estimating the chlorine content in commercial bleaching powder and water.
Organic chemistry
Alkylation of sodium thiosulfate gives S-alkylthiosulfates, which are called Bunte salts.[18] The alkylthiosulfates are susceptible to hydrolysis, affording the thiol. This reaction is illustrated by one synthesis of thioglycolic acid:
- ClCH
2CO
2H + Na
2S
2O
3 → Na[O
3S
2CH
2CO
2H] + NaCl - Na[O
3S
2CH
2CO
2H] + H
2O → HSCH
2CO
2H + NaHSO
4
Safety
Sodium thiosulfate has low toxicity. LDLo for rabbits is 4000 mg/kg.[2]
References
- ↑ Record in the GESTIS Substance Database of the Institute for Occupational Safety and Health
- ↑ 2.0 2.1 2.2 2.3 2.4 2.5 2.6 2.7 "Ullmann's Encyclopedia of Industrial Chemistry". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a25_477.
- ↑ 3.0 3.1 WHO Model Formulary 2008. World Health Organization. 2009. p. 66. ISBN 978-92-4-154765-9.
- ↑ World Health Organization model list of essential medicines: 21st list 2019. Geneva: World Health Organization. 2019. WHO/MVP/EMP/IAU/2019.06. License: CC BY-NC-SA 3.0 IGO.
- ↑ World Health Organization model list of essential medicines: 22nd list (2021). Geneva: World Health Organization. 2021. WHO/MHP/HPS/EML/2021.02.
- ↑ "Tinea versicolor". Int. J. Dermatol. 37 (9): 648–55. 2002. doi:10.1046/j.1365-4362.1998.00441.x. PMID 9762812.
- ↑ "Treatment of Cutaneous Calciphylaxis with Sodium Thiosulfate: Two Case Reports and a Review of the Literature". Am. J. Clin. Dermatol. 12 (5): 339–46. 2011. doi:10.2165/11587060-000000000-00000. PMID 21834598.
- ↑ "Sodium thiosulfate for prevention of cisplatin-induced hearing loss: updated survival from ACCL0431". The Lancet. Oncology 23 (5): 570–572. May 2022. doi:10.1016/S1470-2045(22)00155-3. PMID 35489339.
- ↑ "Protection against Cisplatin-Induced Toxicities by N-Acetylcysteine and Sodium Thiosulfate as Assessed at the Molecular, Cellular, and in Vivo Levels". J. Pharmacol. Exp. Ther. 314 (3): 1052–8. 2005. doi:10.1124/jpet.105.087601. PMID 15951398.
- ↑ Winstead, Edward (October 6, 2022). "Sodium Thiosulfate Reduces Hearing Loss in Kids with Cancer". https://www.cancer.gov/news-events/cancer-currents-blog/2022/fda-sodium-thiosulfate-cisplatin-hearing-loss-children.
- ↑ "FDA approves sodium thiosulfate to reduce the risk of ototoxicity associated with cisplatin in pediatric patients with localized, non-metastatic solid tumors". 20 September 2022. https://www.fda.gov/drugs/resources-information-approved-drugs/fda-approves-sodium-thiosulfate-reduce-risk-ototoxicity-associated-cisplatin-pediatric-patients.
- ↑ The Romance of Modern Photography, Its Discovery & Its Achievements. Seeley & Co. 1908. pp. 37. https://archive.org/details/romancemodernph00gibsgoog. "hyposulphite-of-soda herschel fixer hypo."
- ↑ 13.0 13.1 Inorganic Chemistry. San Diego: Academic Press. 2001. ISBN 978-0-12-352651-9.
- ↑ Elementary Chemistry. 1. Inorganic Chemistry. Chicago: Medico-Dental Publishing Co.. 1913. pp. 162 & 287–288. https://books.google.com/books?id=FgfnAAAAMAAJ&q=sodium+thiosulfate&pg=PA287.
- ↑ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.
- ↑ "Thiosulfate Leaching of Gold - a Review". Minerals Engineering 14 (2): 135–174. 2001. doi:10.1016/s0892-6875(00)00172-2.
- ↑ Малусел, Виорел Александру. "TECHNOLOGY OF GOLD AND SILVER EXTRACTION". https://patents.google.com/patent/EA201370203A1/en.
- ↑ "Sulfide Synthesis in Preparation of Unsymmetrical Dialkyl Disulfides: Sec-butyl Isopropyl Disulfide". Org. Synth. 58: 147. 1978. doi:10.15227/orgsyn.058.0147.
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