Hydrogen Peroxide Chemical Formula
Hydrogen peroxide molecule has molecular formula H2O2 having an interesting gouache structural unit uses widely in industrial solutions and antiseptic or mouth cleaner in medicine. Due to the oxidizing properties of pure hydrogen peroxide, the chemical solution uses as a bleaching product and liquid solution widely uses in textiles work, paper, pump, lather, and oil industry in our everyday life. Hydrogen peroxide is mainly prepared by the electrolysis of concentrated sulfuric acid by the vacuum distillation process.
In hydrogen peroxide structure, two O-H planes lie perpendicular to each other but the solid structural formula is slightly modified by intermolecular hydrogen bonding.
The valence shell electronic configuration of oxygen shows that pz-orbitals oxygen conation a single electron in each orbital in hydrogen peroxide molecule. Therefore, oxygen forms O-O linkages by using the pz-orbitals of the two oxygen atom. The two oxygen atoms form another covalent bonding with the hydrogen atom.
Preparation of Hydrogen Peroxide
Hydrogen Peroxide by Electrolysis
Hydrogen peroxide makes by electrolysis of 50% sulfuric acid followed by careful vacuum distillation. In this process, H2S2O8 acid was first formed by anodic oxidation which hydrolyzed to form H2SO5 and then to H2O2. At the anode, H2SO4 → H+ + HSO4– or, 2HSO4– → H2S2O8 + 2e. At cathode, 2H+ + 2e → H2. In hydrolysis, H2S2O8 + H2O → H2SO5 + H2SO4, and H2SO5 + H2O → H2O2 + H2SO4.
Pure hydrogen peroxide molecule is an extremely pale blue liquid, melting point = -0.43°C, and boiling point = 150°C. The specific heat of formation of liquid H2O2 = -187 kJ mol-1. Therefore, the properties of hydrogen peroxide are unstable due to thermodynamics decomposition like H2O2 (l) → H2O (l) + [O]. However, at the ordinary temperature, the decomposition is very slow but rapidly at a high temp. Thus H2O2 kept preferably in polythene containers which stabilize like urea or phosphoric acid.
The chemical solution of hydrogen peroxide behaves like a weak dibasic acid but the pH scale is lower than water with oxidizing and reducing properties.
H2O2 → H+ + HO2– pKa (200C) = 11.75
H2O2 behaves as a strong oxidant in both acid and base solutions. Therefore, the oxidation reduction potentials for the redox reactions
H2O2 + 2H+ + 2e → 2H2O (1.77 volt)
HO2– +H2O + 2e → 3OH– (087 volt)
2Fe+2 + H2O2 +2H+ → 2Fe+3 + 2H2O
2I– + H2O2 + 2H+ → I2 + 2H2O
In the presence of very strong oxidizing agents such as chlorine or permanganate or dichromate in acid solution, H2O2 oxidizes to form oxygen. In other situations, H2O2 acts as a reducing agent.
Cl2 + H2O2 → 2HCl + O2
Uses of Hydrogen Peroxide Solution
Industrial peroxide is widely used in medicine and bleaching agent in our everyday life. About 30% of peroxide used as a bleaching agent for textiles, paper, pump, later, oils, a large quantity of about 33% uses in the manufacture of borax, epoxides, propylene oxide, and other chemicals. In environmental science, peroxide use in pollution control for the treatment of sewage cleanup and wastes. Hydrogen peroxide uses as a mild antiseptic to prevent the small cut, scapes, and buns on the skin and also use as a mouth rinse in medicine to the freshness or as a mouth cleaner.