Difference between revisions of "Sodium pyrosulfate"
| (3 intermediate revisions by the same user not shown) | |||
| Line 64: | Line 64: | ||
| pKa = | | pKa = | ||
| pKb = | | pKb = | ||
| − | | Solubility = | + | | Solubility = Hydrolyzes |
| SolubleOther = | | SolubleOther = | ||
| Solvent = | | Solvent = | ||
| Line 88: | Line 88: | ||
}} | }} | ||
| Section6 = {{Chembox Hazards | | Section6 = {{Chembox Hazards | ||
| − | | AutoignitionPt = | + | | AutoignitionPt = Non-flammable |
| − | | ExploLimits = | + | | ExploLimits = Non-explosive |
| − | | ExternalMSDS = | + | | ExternalMSDS = None |
| − | | FlashPt = | + | | FlashPt = Non-flammable |
| LD50 = | | LD50 = | ||
| LC50 = | | LC50 = | ||
| Line 105: | Line 105: | ||
| OtherFunction = | | OtherFunction = | ||
| OtherFunction_label = | | OtherFunction_label = | ||
| − | | OtherCompounds = [[Sodium bisulfate]]<br>[[Sodium metabisulfite]] | + | | OtherCompounds = [[Sodium bisulfate]]<br>[[Sodium metabisulfite]]<br>[[Sodium persulfate]] |
}} | }} | ||
}} | }} | ||
| Line 116: | Line 116: | ||
: Na<sub>2</sub>S<sub>2</sub>O<sub>7</sub> → Na<sub>2</sub>SO<sub>4</sub> + SO<sub>3</sub> | : Na<sub>2</sub>S<sub>2</sub>O<sub>7</sub> → Na<sub>2</sub>SO<sub>4</sub> + SO<sub>3</sub> | ||
| − | This reaction is a convenient way of obtaining sulfur trioxide, as it does not require complex | + | This reaction is a convenient way of obtaining sulfur trioxide, as it does not require complex installation and the pyrosulfate precursor, sodium bisulfate, is readily available. |
| + | |||
| + | Sodium pyrosulfate hydrolyzes in water to sulfuric acid.<ref>https://pubs.acs.org/doi/abs/10.1021/ic50004a019</ref> | ||
===Physical=== | ===Physical=== | ||
| Line 137: | Line 139: | ||
==Handling== | ==Handling== | ||
===Safety=== | ===Safety=== | ||
| + | Sodium pyrosulfate rapidly hydrolyzes in contact with water, releasing sulfuric acid, which is corrosive. | ||
===Storage=== | ===Storage=== | ||
| − | In closed bottles. | + | In closed bottles, away from any moisture. |
===Disposal=== | ===Disposal=== | ||
| − | + | Add it in large amounts of water to hydrolyze it, then carefully neutralize the acid with a base. | |
==References== | ==References== | ||
| Line 154: | Line 157: | ||
[[Category:Pyrosulfates]] | [[Category:Pyrosulfates]] | ||
[[Category:Oxidizing agents]] | [[Category:Oxidizing agents]] | ||
| + | [[Category:Materials that react with water]] | ||
Latest revision as of 22:37, 31 March 2019
 |
This article is a stub. Please help Sciencemadness Wiki by expanding it, adding pictures, and improving existing text.
|
| Names | |
|---|---|
| IUPAC name
Disodium disulfate
| |
| Other names
Disulfuric acid disodium salt
Sodium disulfate Sodium pyrosulphate | |
| Identifiers | |
| Jmol-3D images | Image |
| |
| Properties | |
| Na2S2O7 | |
| Molar mass | 222.12 g/mol |
| Appearance | White crystalline solid |
| Density | 2.658 g/cm3 |
| Melting point | 400.9 °C (753.6 °F; 674.0 K) |
| Boiling point | 460 °C (860 °F; 733 K) (decomposition) |
| Hydrolyzes | |
| Thermochemistry | |
| Std enthalpy of
formation (ΔfH |
-1,717.6--1,907 kJ/mol |
| Hazards | |
| Safety data sheet | None |
| Flash point | Non-flammable |
| Related compounds | |
| Related compounds
|
Sodium bisulfate Sodium metabisulfite Sodium persulfate |
| Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
| Infobox references | |
Sodium pyrosulfate (also known as disodium disulfate) is a sodium salt of disulfuric acid, with the formula Na2S2O7.
Contents
Properties
Chemical
Sodium pyrosulfate decomposes when heated above 460 °C to give sodium sulfate and sulfur trioxide:
- Na2S2O7 → Na2SO4 + SO3
This reaction is a convenient way of obtaining sulfur trioxide, as it does not require complex installation and the pyrosulfate precursor, sodium bisulfate, is readily available.
Sodium pyrosulfate hydrolyzes in water to sulfuric acid.[1]
Physical
Sodium disulfate is a white salt, soluble in water.
Availability
Sodium pyrosulfate is rarely available from suppliers. Sigmaaldrich used to sell sodium disulfate fused with sodium bisulfate.
Preparation
Sodium pyrosulfate can be easily made by heating sodium bisulfate at temperatures between 200-400 °C:
- 2 NaHSO4 → Na2S2O7 + H2O
However, other authors indicate different temperature decomposition ranges.[2]
Projects
- Make sulfur trioxide
- Make ammonium pyrosulfate
Handling
Safety
Sodium pyrosulfate rapidly hydrolyzes in contact with water, releasing sulfuric acid, which is corrosive.
Storage
In closed bottles, away from any moisture.
Disposal
Add it in large amounts of water to hydrolyze it, then carefully neutralize the acid with a base.
References
- ↑ https://pubs.acs.org/doi/abs/10.1021/ic50004a019
- ↑ http://doc.utwente.nl/68103/1/Vries69thermal.pdf
Relevant Sciencemadness threads
- Article stubs
- Chemical pages without CAS Registry Number
- Articles without EBI source
- Chemical pages without ChemSpiderID
- Chemical pages without DrugBank identifier
- Articles without KEGG source
- Articles without InChI source
- Articles without UNII source
- Articles containing unverified chemical infoboxes
- Chembox articles without image
- Chemical compounds
- Inorganic compounds
- Sodium compounds
- Pyrosulfates
- Oxidizing agents
- Materials that react with water
