Sodium perchlorate sample
| IUPAC name
| Other names
|Molar mass||122.44 g/mol|
|Appearance||White crystalline solid|
|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|
|Safety data sheet|| ScienceLab (anhydrous)|
| Sodium hypochlorite|
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Sodium perchlorate is an inorganic salt of sodium, with the chemical formula NaClO4.
Sodium perchlorate is a powerful oxidizer, though it's not as useful in pyrotechnics as the potassium salt due to its hygroscopicity.
- NaClO4(aq) + H2SO4(aq) ↔ NaHSO4 (aq) + HClO4(aq)
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.
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.
- 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 50g/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.
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.
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.
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.
Sodium perchlorate should not be poured down the drain or dumped into environment. It must be neutralized with a reducing agent to NaCl first.
- Liptakov's video on producing sodium perchlorate from sodium chlorate by thermal decomposition: https://www.youtube.com/watch?v=1Ylt2ZKJlME
- Perchlorate in the Environment (2000), Edward Todd Urbansky, pag. 106