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The introduction of the electrical dynamo in the early 1870s made large scale, relatively inexpensive electric power available for commercial scale chemical production.

Association constant of vanadium (11I) with sulfate ion was determined by measuring ab-sorbance of vanadium OE in sulfuric or perchloric acid of various concentrations. Kvs04,-CVSO4+NEV3÷1[SO42-1) at 25°C has been found to be 29 through the photometric measurement at 400 nm under the following conditions: EVOR)ltotai = 8.2 mmol/l, [1-1+] = 0.85 moIll, [H2SO4] =0.083,-0.664molg and /i (ionic strength)= 1.0, and to be 28 through the photometric measurement at 250 nm under the following conditions: EV(II)itotal = 0.93, mmol/l, [1-1+] = 0.92, [H2SO4] =0 .0126-'0.0766 mol/l and ,u=1.0,. Moreover, the molecular extinction coefficients of V3+ and VSO4+ have been estimated in the regions of 230-280 nm and 350-'700 nm.

Electrochemical processes are used to produce an array of reactive inorganic chemicals and metals. The most reactive materials, strongest oxidants, and strongest reductants are produced electrochemically at anodes and cathodes, respectively. Process technology for the production of each electrochemical is unique. Power supplies and electrolytic cells are the distinguishing features of electrochemical processes. Electrolytic cells use direct current and are designed to be process specific. Every cell consists of an anode, a cathode, and container. Cells may be monopolar or bipolar, with or without separators, and equipped to handle aqueous solutions or fused salt electrolytes. Industrial processes described include electrolysis of chloride solutions and production of manganese dioxide, fluorine, permanganate, and hydrogen peroxide. The electrolysis of water and production of heavy water are also described. Processes for electrowinning of metals from aqueous solutions and from fused salts are discussed as are electrochemical processes for hazardous waste treatment systems.

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