Barium azide

<h2 id="preparation">Preparation</h2>
<p>Barium azide may be prepared by reacting <a href="/facts/Sodium_azide/4gwc2jzu">sodium azide</a> with a soluble barium salt:<a class="footnote-ref" id="fnref:1" href="#fn:1"><sup>1</sup></a>
</p>
BaBr2 +  2 NaN3   →   Ba(N3)2  +  2NaBr
<h2 id="uses">Uses</h2>
<p>Barium azide can be used to make azides of <a href="/facts/Magnesium_azide/LTVE3ev6">magnesium</a>, <a href="/facts/Sodium_azide/4gwc2jzu">sodium</a>, <a href="/facts/Potassium_azide/G1f5yGe7">potassium</a>, <a href="/facts/Lithium_azide/4S1YV1VA">lithium</a>, <a href="/facts/Rubidium_azide/E84aVIfK">rubidium</a> and <a href="/facts/Zinc_azide/7dYbYShx">zinc</a> with their respective sulfates.<a class="footnote-ref" id="fnref:2" href="#fn:2"><sup>2</sup></a>
</p>
Ba(N3)2 + Li2SO4 → 2 LiN3 + BaSO4
<p>It can also be used as a source for high purity nitrogen by heating:
</p>
Ba(N3)2 → Ba + 3 N2
<p>This reaction liberates metallic barium, which is used as a <a href="/facts/Getter/xYE7jToy">getter</a> in vacuum applications.
</p>
<h2 id="see-also">See also</h2>
<ul><li><a href="/facts/Calcium_azide/E5D7L6XL">Calcium azide</a></li>
<li><a href="/facts/Sodium_azide/4gwc2jzu">Sodium azide</a></li>
<li><a href="/facts/Hydrazoic_acid/rbtF5smp">Hydrazoic acid</a></li></ul>

<h2 id="references">References</h2>

<ol>
<li id="fn:1"><p>Jobelius, Horst H.; Scharff, Hans-Dieter (2000). "Hydrazoic Acid and Azides". Ullmann's Encyclopedia of Industrial Chemistry. Wiley-VCH. doi:10.1002/14356007.a13_193. ISBN 9783527306732. <a href="9783527306732" target="_blank">9783527306732</a> <a href="#fnref:1" class="footnote-back-ref">↩</a></p></li>
<li id="fn:2"><p>H. D. Fair; R. F. Walker, eds. (1977). Physics and Chemistry of the Inorganic Azides. Energetic Materials. Vol. 1. New York and London: Plenum Press. ISBN 9781489950093. <a href="9781489950093" target="_blank">9781489950093</a> <a href="#fnref:2" class="footnote-back-ref">↩</a></p></li>
</ol>

Barium azide open-in-new

Barium azide