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Nov 28

All About Chemistry is a free website that covers chemistry syllabus from class 8 to 12, JEE, NEET, Graduation, and Masters Degree level.Theme pic By Ayan Rahman. You have entered an incorrect email address! Its boiling point has been determined to be 423.2 extrapolation method. 2) The two oxygen atoms are linked to each other by a single covalent bond and each oxygen is further linked to a hydrogen atom by a single covalent bond. 10H2O) which is removed by filtration. b) By the action of carbon dioxide or carbonic acid : When a rapid stream of CO2 is bubbled through a thin paste of BaO2 in ice cold water, H2O2 and BaCO3 are produced. 2) It oxidises manganese salts to manganese dioxide, MnSO4 + 2NaOH + H2O2 ———-> Na2SO4 + MnO4 + 2H2O, 3) It oxidises ferrous salts to ferric salts, 2FeSO4 + 4NaOH + H2O2 ———->2 Fe(OH)3 + 2 Na2SO4, 4)It oxidises Chromium salts to chromates, Cr2(SO4)3 +3H2O2  + 10 NaOH———-> 2 Na2CrO4 + 3 Na2SO4 + 8H2O, 5) It oxidises formaldehyde to formic acid. It is example of auto oxidation and auto reduction. Advantage : Since almost all the heavy metals impurities present in BaO2 and which catalyse the decomposition of hydrogen peroxide are removed as insoluble phosphates.As a result ,the resulting solution of hydrogen peroxide has good keeping properties. These crystals are then, removed, dried, and melted. Anhydrous barium peroxide cannot be used since the precipitated BaSO4 forms a protective layer around unreacted barium peroxide thereby preventing the further reaction. It is used to restore the colour of old lead paints. Hydrogen peroxide was discovered by the French chemist J.L.Thenard in 1818. 1) Hydrogen peroxide cannot be stored in glass bottles since the rough surface of glass ,alkali oxides present in it, and exposure to light catalyse its decomposition. 9) It is used in laboratory for detecting the presence of chromium ,titanium and vanadium salts with which it yields peroxides of characteristic colours. It is used for bleaching silk, paper pulp, ivory,hairetc. 3) The two O-H bonds are however in different planes due to repulsion between different bonding and antibonding orbitals. 8) It is used for restoring the colour of lead painting which have blackened due to action of H2S present in the air on lead paints. The temperature of the acid and barium peroxide is kept at 0, Hydrogen peroxide can also be prepared from barium peroxide by rapidly bubbling carbon dioxide through a thin paste of BaO. Hydrogen peroxide adds with ethane to produce Ethylene glycol, In the above process anhydrous barium peroxide is not taken as it form an insoluble coating of barium sulphate and stops the further reaction. Therefore hydrogen peroxide is usually stored in coloured paraffin wax coated plastic or teflon bottles. 5)Charcoal. In presence of strong oxidising agent, hydrogen peroxide behave as a reducing agent in acidic as well as alkaline medium.In these reactions, molecular oxygen is always produced by the combination of H2O2with the oxygen atom released by the strong oxidising agent. Chemical Properties: Hydrogen peroxide in both acidic and basic medium acts as an oxidizing as well as the reducing agent. Pure hydrogen peroxide turns blue litmus red but its dilute solution is neutral to litmus. 4) In the production of epoxides ,propylene oxide and polyurethane. It is used to produce spongy rubber, hydroquinone, sodium percarbonate, sodium perborate, polyurethanes, epoxides, tartaric acid, cephalosoporin, propylene oxide etc. Thanks Now ice cold paste is slowly added to ice cold dilute sulphuric acid by constantly stirring with a glass rod till the final solution remains slightly acidic. Pressure inside the desiccator is reduced by connecting it to a vacuum pump. Hydrogen peroxide cannot be concentrated simply by distillation since its decomposers much below its boiling point to give water and oxygen. 2HSO4– – 2e– → H2S2O8(Peroxodisulphuric acid). Hydrogen peroxide has an open book structure .Two oxygen atoms remain bonded to each other by peroxide linkage (-O-O-). 1) Hydrogen peroxide is a non – planar molecule. __________________________________________________________, 2 MnO4‾ + 6 H+ + 5 H2O2 ——-> 2Mn2+ + 8 H2O + 5O2. Sulphuric acid cannot be used the above process as it oxidises H, Nitric acid cannot be used in the above process as it oxidizes H. The final solution produced in the above reaction is kept slightly acidic as acid acts as a negative catalyst in the decomposition of hydrogen peroxide.

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