Sodium perchlorate

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Sodium perchlorate is an inorganic salt of sodium, with the chemical formula NaClO₄.

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 careful 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.

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 sodium chloride) at an inert electrode, such as platinum.

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.

Projects

• Make potassium perchlorate
• 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.

Disposal

Sodium perchlorate should not be poured down the drain or dumped into environment. It must be neutralized with a reducing agent first.

References

Relevant Sciencemadness threads

• pH control of a Sodium Perchlorate cell
• Seeking help regarding unsuccessful sodium perchlorate cell