Difference between revisions of "Sodium perchlorate"
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| Section6 = {{Chembox Hazards | | Section6 = {{Chembox Hazards | ||
| AutoignitionPt = Non-flammable | | AutoignitionPt = Non-flammable | ||
| − | | ExploLimits = | + | | ExploLimits = Non-flammable |
| ExternalMSDS = [http://www.sciencelab.com/msds.php?msdsId=9925018 ScienceLab] (anhydrous)<br>[http://www.sciencelab.com/msds.php?msdsId=9927599 ScienceLab] (monohydrate) | | ExternalMSDS = [http://www.sciencelab.com/msds.php?msdsId=9925018 ScienceLab] (anhydrous)<br>[http://www.sciencelab.com/msds.php?msdsId=9927599 ScienceLab] (monohydrate) | ||
| FlashPt = Non-flammable | | FlashPt = Non-flammable | ||
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: ClO<sub>3</sub><sup>-</sup> (aq) + H<sub>2</sub>O (l) → ClO<sub>4</sub><sup>-</sup> (aq) + H<sub>2</sub> (g) | : ClO<sub>3</sub><sup>-</sup> (aq) + H<sub>2</sub>O (l) → ClO<sub>4</sub><sup>-</sup> (aq) + H<sub>2</sub> (g) | ||
| − | However when using platinum as an anode, its wear rate will increase as the chlorate concentration starts to decrease, and below | + | However when using platinum as an anode, its wear rate will increase as the chlorate concentration starts to decrease, and below 50 g/l it may be excessive; high temperatures also increase its wear rate. Wear rates from manufacturers have been reported as 3 to 6 grams of Pt per ton of sodium perchlorate.<ref>http://www.oocities.org/capecanaveral/campus/5361/chlorate/naperchl.html</ref> |
Sodium perchlorate can also be prepared by thermal decomposition of sodium chlorate, yielding sodium chloride as side product. Since the sodium perchlorate can also decompose and the sodium chlorate can give off oxygen without making perchlorate, this can be a lossy way to produce this compound. | Sodium perchlorate can also be prepared by thermal decomposition of sodium chlorate, yielding sodium chloride as side product. Since the sodium perchlorate can also decompose and the sodium chlorate can give off oxygen without making perchlorate, this can be a lossy way to produce this compound. | ||
Revision as of 15:42, 2 December 2022
 Sodium perchlorate sample
| |
| |
| Names | |
|---|---|
| IUPAC name
Sodium perchlorate
| |
| Other names
Sodium chlorate(VII)
Sodium hyperchlorate | |
| Identifiers | |
| Jmol-3D images | Image |
| |
| Properties | |
| NaClO4 | |
| Molar mass | 122.44 g/mol |
| Appearance | White crystalline solid |
| Odor | Odorless |
| Density | 2.4994 g/cm3 (anhydrous) 2.02 g/cm3 (monohydrate) |
| Melting point | 468 °C (874 °F; 741 K) (decomposes, anhydrous) 130 °C (266 °F; 403.15 K) (monohydrate) |
| Boiling point | 482 °C (900 °F; 755 K) (monohydrate, decomposes) |
| 209.6 g/100 ml (25 °C, anhydrous) 209 g/100 ml (15 °C, monohydrate) | |
| Solubility | Soluble in acetone Insoluble in benzene, chloroform, toluene |
| Solubility in acetone | 52 g/100 g |
| Vapor pressure | ~0 mmHg |
| Hazards | |
| Safety data sheet | ScienceLab (anhydrous) ScienceLab (monohydrate) |
| Flash point | Non-flammable |
| Related compounds | |
| Related compounds
|
Sodium hypochlorite Sodium chlorite Sodium chlorate |
| Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
| Infobox references | |
Sodium perchlorate is an inorganic salt of sodium, with the chemical formula NaClO4.
Contents
Properties
Chemical
Sodium perchlorate is a powerful oxidizer, though it's not as useful in pyrotechnics as the potassium salt due to its hygroscopicity.
It will react with a strong mineral acid, such as sulfuric acid, to form perchloric acid. This can be isolated by vacuum distillation.
- NaClO4(aq) + H2SO4(aq) ↔ NaHSO4 (aq) + HClO4(aq)
Physical
Sodium perchlorate is a white crystalline salt. It is hygroscopic, forming a monohydrate. It is highly soluble in water, 209 g/100 ml at 25 °C. It is also soluble in low chain alcohols.
Availability
Sodium perchlorate used to be available globally, but recent regulations have restricted its possession in Europe. Perchlorates can still be purchased from some online vendors, but in limited quantities. Purchases using some form of identification have a good chance of being tracked by a government agency. In the US, perchlorates are still widely available through pyrotechnic companies as well as lab suppliers.
Preparation
Sodium perchlorate is produced by anodic oxidation of sodium chlorate (which in turn is made from the electrolysis of a solution of sodium chloride) at an inert electrode, such as platinum.[1]
- ClO3- (aq) + H2O (l) → ClO4- (aq) + H2 (g)
However when using platinum as an anode, its wear rate will increase as the chlorate concentration starts to decrease, and below 50 g/l it may be excessive; high temperatures also increase its wear rate. Wear rates from manufacturers have been reported as 3 to 6 grams of Pt per ton of sodium perchlorate.[2]
Sodium perchlorate can also be prepared by thermal decomposition of sodium chlorate, yielding sodium chloride as side product. Since the sodium perchlorate can also decompose and the sodium chlorate can give off oxygen without making perchlorate, this can be a lossy way to produce this compound.
- 4 NaClO3 → NaCl + 3 NaClO4
The reaction is considerably faster than a perchlorate cell however. The main drawbacks are the difficulty in holding the temperature (since sodium perchlorate also decomposes) and the danger of the molten chlorate. It is doubtful if this method scales well. The resulting reaction mixture can be separated by dissolution of the perchlorate in acetone, since both sodium chlorate and sodium chloride are rather poorly soluble in it.[3][4]
Projects
- Make potassium perchlorate
- Make perchloric acid
- Flash powder
- Chemical oxygen generator
Handling
Safety
Sodium perchlorate is a powerful oxidizer. It should be kept away from organic substances and strong reducing agents. Unlike chlorates, perchlorate mixtures with sulfur are relatively stable.
It is moderately toxic, as in large amounts it interferes with iodine uptake into the thyroid gland.
Storage
NaClO4 should be stored in tightly sealed bottles as it is slightly hygroscopic. It should be kept away from any strong acidic vapors to prevent the formation of anhydrous perchloric acid, a fire and explosion hazard. It must also be kept away from any flammable materials.
Disposal
Sodium perchlorate should not be poured down the drain or dumped into environment. It must be neutralized with a reducing agent to NaCl first.
Sodium perchlorate can be destroyed with metallic iron under UV light, in the absence of air.[5]
Gallery
Sodium perchlorate crystals forming in acetone solution.
References
- ↑ http://www.utahpyro.org/compositions/HowToMakeSodiumPerchlorate.pdf
- ↑ http://www.oocities.org/capecanaveral/campus/5361/chlorate/naperchl.html
- ↑ Liptakov's video on producing sodium perchlorate from sodium chlorate by thermal decomposition: https://www.youtube.com/watch?v=1Ylt2ZKJlME
- ↑ https://patents.google.com/patent/US3151935A/en
- ↑ Perchlorate in the Environment (2000), Edward Todd Urbansky, pag. 106
Relevant Sciencemadness threads
- 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
- Chemical compounds
- Inorganic compounds
- Oxidizing agents
- Sodium compounds
- Perchlorates
- Neutral salts
