Difference between revisions of "Sodium thiosulfate"
From Sciencemadness Wiki
(→Disposal) |
|||
| (11 intermediate revisions by 3 users not shown) | |||
| Line 1: | Line 1: | ||
{{Chembox | {{Chembox | ||
| − | | Name =Sodium thiosulfate | + | | Name = Sodium thiosulfate |
| Reference = | | Reference = | ||
| − | | IUPACName =Sodium thiosulfate | + | | IUPACName = Sodium thiosulfate |
| − | | PIN = | + | | PIN = |
| − | | SystematicName =Sodium thiosulfate | + | | SystematicName = Sodium thiosulfate |
| − | | OtherNames = | + | | OtherNames = Sodium thiosulphate<br>Sodium hyposulfite<br>Hyposulphite of soda |
| − | + | ||
| − | + | ||
| − | + | ||
| − | + | ||
<!-- Images --> | <!-- Images --> | ||
| − | | ImageFile = | + | | ImageFile = Sodium thiosulfate sample watchglass.jpg |
| − | | ImageSize = | + | | ImageSize = 300 |
| ImageAlt = | | ImageAlt = | ||
| ImageName = | | ImageName = | ||
| + | | ImageCaption = Sodium thiosulfate pentahydrate crystals | ||
| ImageFile1 = | | ImageFile1 = | ||
| ImageSize1 = | | ImageSize1 = | ||
| Line 65: | Line 62: | ||
| MeltingPt_ref = | | MeltingPt_ref = | ||
| MeltingPt_notes = (pentahydrate) | | MeltingPt_notes = (pentahydrate) | ||
| + | | Odor = Odorless | ||
| pKa = | | pKa = | ||
| pKb = | | pKb = | ||
| Solubility = 70.1 g/100 mL (20 °C)<br>231 g/100 mL (100 °C) | | Solubility = 70.1 g/100 mL (20 °C)<br>231 g/100 mL (100 °C) | ||
| − | | SolubleOther = | + | | SolubleOther = Almost insoluble in [[acetonitrile]], [[ethanol]], [[methanol]] |
| Solvent = | | Solvent = | ||
| − | | VaporPressure = | + | | VaporPressure = ~ 0 mmHg |
}} | }} | ||
| Section3 = {{Chembox Structure | | Section3 = {{Chembox Structure | ||
| Line 97: | Line 95: | ||
| LD50 = | | LD50 = | ||
| LC50 = | | LC50 = | ||
| − | | MainHazards = | + | | MainHazards = Irritant |
| NFPA-F = | | NFPA-F = | ||
| NFPA-H = | | NFPA-H = | ||
| Line 108: | Line 106: | ||
| OtherFunction = | | OtherFunction = | ||
| OtherFunction_label = | | OtherFunction_label = | ||
| − | | OtherCompounds = | + | | OtherCompounds = [[Ammonium thiosulfate]]<br>[[Sodium metabisulfite]]<br>[[Sodium sulfite]] |
}} | }} | ||
}} | }} | ||
| − | '''Sodium thiosulfate''' is an inorganic compound with the chemical formula Na<sub>2</sub>S<sub>2</sub>O<sub>3</sub>. The solid is | + | '''Sodium thiosulfate''' is an inorganic compound with the chemical formula '''Na<sub>2</sub>S<sub>2</sub>O<sub>3</sub>''', widely used in titrations and as cyanide poisoning antidote. The most common form of this salt is the pentahydrate '''Na<sub>2</sub>S<sub>2</sub>O<sub>3</sub>·5H<sub>2</sub>O'''. This solid is slightly efflorescent. |
==Properties== | ==Properties== | ||
===Chemical=== | ===Chemical=== | ||
Sodium thiosulfate reacts with acids, releasing sulfur, and sulfur dioxide fumes: | Sodium thiosulfate reacts with acids, releasing sulfur, and sulfur dioxide fumes: | ||
| − | |||
| − | + | : Na<sub>2</sub>S<sub>2</sub>O<sub>3</sub> + 2 HCl → 2 NaCl + S + SO<sub>2</sub> + H<sub>2</sub>O | |
| − | :4 Na<sub>2</sub>S<sub>2</sub>O<sub>3</sub> → 3 Na<sub>2</sub>SO<sub>4</sub> + Na<sub>2</sub>S<sub>5</sub> | + | The hydrated form has a low melting point of around 50 °C, but in fact it decomposes and the salt dissolves in its own water of crystallization. When heated more strongly, the water is driven off. When the anhydrous compound is heated to 300 °C, it decomposes to [[sodium sulfate]] and sodium polysulfide: |
| + | |||
| + | : 4 Na<sub>2</sub>S<sub>2</sub>O<sub>3</sub> → 3 Na<sub>2</sub>SO<sub>4</sub> + Na<sub>2</sub>S<sub>5</sub> | ||
===Physical=== | ===Physical=== | ||
| − | Sodium thiosulfate is an odorless white crystalline solid, soluble in water, but almost insoluble in alcohols. | + | Sodium thiosulfate pentahydrate is an odorless white crystalline solid, soluble in water, but almost insoluble in alcohols. |
==Availability== | ==Availability== | ||
| − | Sodium thiosulfate is sometimes sold in pharmacies or pet stores. | + | Sodium thiosulfate pentahydrate is sold by many swimming pool suppliers, as "chlorine neutralizer", in solid form. |
| + | |||
| + | Sodium thiosulfate is sometimes sold in pharmacies or pet stores. It can be bought cheaply online. | ||
==Preparation== | ==Preparation== | ||
| − | Sodium thiosulfate can be prepared by boiling an aqueous [[sodium hydroxide]] solution with elemental [[sulfur]]. | + | Sodium thiosulfate can be prepared by boiling an aqueous [[sodium hydroxide]] solution with elemental [[sulfur]], but isolation of the pure solid compound is not easy. The other reaction product is sulfide and polysulfide. |
| − | [[Sodium sulfite]] can also be used instead of sodium hydroxide. | + | [[Sodium sulfite]] can also be used instead of sodium hydroxide. In that case, the only reaction product is sodium thiosulfate. |
==Projects== | ==Projects== | ||
*Iodine clock reaction | *Iodine clock reaction | ||
| − | *Neutralize bleach | + | *Neutralize [[bleach]] |
*Remove [[iodine]] stains | *Remove [[iodine]] stains | ||
*Cyanide poisoning antidote | *Cyanide poisoning antidote | ||
| − | *Gold extraction | + | *[[Gold]] extraction |
*Supercooling demonstration | *Supercooling demonstration | ||
*Redox titrations | *Redox titrations | ||
*Bunte salts synthesis | *Bunte salts synthesis | ||
| − | *Thioglycolic acid synthesis | + | *[[Thioglycolic acid]] synthesis |
==Handling== | ==Handling== | ||
| Line 149: | Line 150: | ||
===Storage=== | ===Storage=== | ||
| − | + | Sodium thiosulfate should be kept in closed containers. | |
===Disposal=== | ===Disposal=== | ||
| − | + | No special precautions need to be taken. Bleach can be used to neutralize it. | |
==References== | ==References== | ||
| Line 166: | Line 167: | ||
[[Category:Reducing agents]] | [[Category:Reducing agents]] | ||
[[Category:Materials unstable in acidic solution]] | [[Category:Materials unstable in acidic solution]] | ||
| + | [[Category:Readily available chemicals]] | ||
[[Category:Materials available as food grade]] | [[Category:Materials available as food grade]] | ||
| + | [[Category:Antidotes]] | ||
Latest revision as of 22:41, 17 October 2020
 Sodium thiosulfate pentahydrate crystals
| |
| Names | |
|---|---|
| IUPAC name
Sodium thiosulfate
| |
| Systematic IUPAC name
Sodium thiosulfate | |
| Other names
Sodium thiosulphate
Sodium hyposulfite Hyposulphite of soda | |
| Properties | |
| Na2S2O3 | |
| Molar mass | 158.11 g/mol (anhydrous) 248.18 g/mol (pentahydrate) |
| Appearance | White crystalline solid |
| Odor | Odorless |
| Density | 1.667 g/cm3 |
| Melting point | 48.3 °C (118.9 °F; 321.4 K) (pentahydrate) |
| Boiling point | 100 °C (pentahydrate) 320 °C (608 °F; 593 K) (decomposes) |
| 70.1 g/100 mL (20 °C) 231 g/100 mL (100 °C) | |
| Solubility | Almost insoluble in acetonitrile, ethanol, methanol |
| Vapor pressure | ~ 0 mmHg |
| Hazards | |
| Safety data sheet | MSDS |
| Flash point | Non-flammable |
| Related compounds | |
| Related compounds
|
Ammonium thiosulfate Sodium metabisulfite Sodium sulfite |
| Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
| Infobox references | |
Sodium thiosulfate is an inorganic compound with the chemical formula Na2S2O3, widely used in titrations and as cyanide poisoning antidote. The most common form of this salt is the pentahydrate Na2S2O3·5H2O. This solid is slightly efflorescent.
Contents
Properties
Chemical
Sodium thiosulfate reacts with acids, releasing sulfur, and sulfur dioxide fumes:
- Na2S2O3 + 2 HCl → 2 NaCl + S + SO2 + H2O
The hydrated form has a low melting point of around 50 °C, but in fact it decomposes and the salt dissolves in its own water of crystallization. When heated more strongly, the water is driven off. When the anhydrous compound is heated to 300 °C, it decomposes to sodium sulfate and sodium polysulfide:
- 4 Na2S2O3 → 3 Na2SO4 + Na2S5
Physical
Sodium thiosulfate pentahydrate is an odorless white crystalline solid, soluble in water, but almost insoluble in alcohols.
Availability
Sodium thiosulfate pentahydrate is sold by many swimming pool suppliers, as "chlorine neutralizer", in solid form.
Sodium thiosulfate is sometimes sold in pharmacies or pet stores. It can be bought cheaply online.
Preparation
Sodium thiosulfate can be prepared by boiling an aqueous sodium hydroxide solution with elemental sulfur, but isolation of the pure solid compound is not easy. The other reaction product is sulfide and polysulfide.
Sodium sulfite can also be used instead of sodium hydroxide. In that case, the only reaction product is sodium thiosulfate.
Projects
- Iodine clock reaction
- Neutralize bleach
- Remove iodine stains
- Cyanide poisoning antidote
- Gold extraction
- Supercooling demonstration
- Redox titrations
- Bunte salts synthesis
- Thioglycolic acid synthesis
Handling
Safety
Sodium thiosulfate may cause irritation on contact.
Storage
Sodium thiosulfate should be kept in closed containers.
Disposal
No special precautions need to be taken. Bleach can be used to neutralize it.
