The Decomposition of Hydrogen Peroxide

In this laboratory exercise we will determine the percentage Hydrogen Peroxide present in a commercially available solution by measuring the volume of Oxygen gas liberated when the peroxide decomposes.  Because the decomposition of dilute solutions of Hydrogen Peroxide is relatively slow, a Ferric Chloride catalyst will be used to increase the reaction rate so that the reaction goes to completion during the laboratory period.   

In its pure form, Hydrogen Peroxide (H2O2) is a faintly bluish, syrupy liquid which boils at 150.2^oC.  It was first synthesized by the French chemist Louis Jaques Thenard in 1818 by acidification of Barium Peroxide (BaO2) with Nitric Acid (HNO3).  This process was supplanted by an improved version in which the Barium Peroxide is initially treated with Hydrochloric Acid (HCl), followed by addition of Sulfuric Acid (H2SO4) to precipitate the Barium Ion (Ba²⁺) as Barium Sulfate (BaSO4). 

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