Difference between revisions of "Sodium perchlorate"

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(Created page with "[File:Sodium perchlorate.jpg|thumb|220x220px]] 220x220px '''Sodium perchlorate''' is an inorganic salt of sodium, with the chem...")
 
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==Properties==
 
==Properties==
 
===Chemical===
 
===Chemical===
−
Sodium perchlorate is a powerful oxidizer, albeit it's not as powerful as its potassium counterpart due to its hygroscopicity.
+
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 [[hydrochloric acid]], to form [[perchloric acid]].
+
It will react with a strong mineral acid, such as [[sulfuric acid]], to form [[perchloric acid]].  This can be isolated by careful distillation.
  
−
:NaClO<sub>4</sub>(aq) + HCl(aq) ↔ NaCl (aq) + HClO<sub>4 </sub>(aq)
+
:NaClO<sub>4</sub>(aq) + H<sub>2</sub>SO<sub>4</sub>(aq) ↔ NaHSO<sub>4</sub> (aq) + HClO<sub>4</sub>(aq)
  
 
===Physical===
 
===Physical===
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==Availability==
 
==Availability==
−
Sodium perchlorate used to be available, but now it's restricted 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. Perchlorates are usually better made than bought, if one can find the correct electrodes.
+
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==
 
==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]].<ref>http://www.utahpyro.org/compositions/HowToMakeSodiumPerchlorate.pdf</ref>
 
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]].<ref>http://www.utahpyro.org/compositions/HowToMakeSodiumPerchlorate.pdf</ref>
  
−
:ClO<sup>3−</sup> (aq) + H<sub>2</sub>O (l) → ClO<sup>4−</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 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.<ref>http://www.oocities.org/capecanaveral/campus/5361/chlorate/naperchl.html</ref>
 
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.<ref>http://www.oocities.org/capecanaveral/campus/5361/chlorate/naperchl.html</ref>
  
 
==Projects==
 
==Projects==
−
*Make [[potassium chlorate]]
+
*Make [[potassium perchlorate]]
 
*Flash powder
 
*Flash powder
 
*Chemical oxygen generator
 
*Chemical oxygen generator
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==Handling==
 
==Handling==
 
===Safety===
 
===Safety===
−
Sodium perchlorate is a powerful oxidizer. It should be kept away from any open flame and organic substances. Unlike the chlorate salt, perchlorate mixtures with sulfur are stable.
+
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.
 
It is moderately toxic, as in large amounts it interferes with iodine uptake into the thyroid gland.
  
 
===Storage===
 
===Storage===
−
NaClO<sub>4</sub> should be stored in closed bottles, sealed preferable, as it is slightly hygroscopic. It must kept away from any strong acidic vapors, to prevent it from releasing perchloric acid, a fire and explosion hazard.
+
NaClO<sub>4</sub> 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===
 
===Disposal===

Revision as of 01:39, 2 November 2015

[File:Sodium perchlorate.jpg|thumb|220x220px]]

File:488px-Sodium perchlorate.svg.png
220x220px

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.[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 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.[2]

Projects

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

  1. ↑ http://www.utahpyro.org/compositions/HowToMakeSodiumPerchlorate.pdf
  2. ↑ http://www.oocities.org/capecanaveral/campus/5361/chlorate/naperchl.html

Relevant Sciencemadness threads

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