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Hydrogen Peroxide
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Hydrogen peroxide 2. From Barium peroxide Barium sulphate is filtered off leaving behind H 2 O 2. Methods of preparation
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3. By electrolysis of 50% H 2 SO 4 H 2 SO 4 At cathode At Anode H 2 O 2 distills first leaving behind the H 2 SO 4 which is recycled.
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4. By auto oxidation of 2- ethylanthraquinol The H 2 O 2 obtained by this method is further concentrated by distillation under reduced pressure.
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Physical Properties In the pure state H 2 O 2 is an almost colourless (very pale blue) liquid. H 2 O 2 is miscible with water in all proportions and forms a hydrate H 2 O 2.H 2 O A 30% solution of H 2 O 2 is marketed as ‘100 volume’ hydrogen peroxide.
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Structure of hydrogen peroxide
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Oxidising properties Chemical Properties
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Oxidising properties
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Reducing properties
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Acidic properties It reacts with alkalies and decomposes carbonates.
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For bleaching silk, wool, hair and leather As rocket fuel Dilute solution is sold in name ‘perhydrol’ It is used in the synthesis of hydroquinone, tartaric acid and certain food products and pharmaceuticals (cephalosporin) etc. Uses of hydrogen peroxide
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H 2 O 2 is stored in the bottles lined with wax because the rough glass surface causes the decomposition of hydrogen peroxide. Storage H 2 O 2 decomposes slowly on exposure to light.
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Volume strength of hydrogen peroxide Calculate the percentage strength of a 10 volume H 2 O 2 solution. 10 volume hydrogen peroxide means that 1 ml of such a solution of hydrogen peroxide on heating will produce 10 ml of oxygen at N.T.P. 2(2 + 32) gm 22.4L at N.T.P. = 68 gm or 22400 cm 3 at N.T.P.
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Solution But 10 ml of O 2 at N.T.P. are produced from 1 ml of 10 volume H 2 O 2 solution. = 0.03035 gm
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Illustrative example Calculate the normality of 30 volume of H 2 O solution: Solution: 2(2 + 32) gm 22.4 L = 68 gm 22.4 L of O 2 is produced from = 68 gm of H 2 O 2 = 91.07 gm/mL
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Solution 68 parts by weight32 parts by weight 32 parts by weight of oxygen is obtained from = 68 parts by weight of H 2 O 2 parts by weight of oxygen is obtained from =
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