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An aqueous solution of NaCl on electroly...

An aqueous solution of `NaCl` on electrolysis gives `H_(2)(g), Cl_(2)(g),` and `NaOH` accroding to the reaction `:`
`2Cl^(-)(aq)+2H_(2)Orarr2overset(-)(O)H(aq)+H_(2)(g)+Cl_(2)(g)`
A direct current of `25A` with a current efficiency of `62%` is passed through `20L` of `NaCl` solution `(20%` by weight`)`. Write down the reactions taking place at the anode and cathode. How long will it take to produce `1 kg ` of `Cl_(2)`? What will be the molarity of the solution with respect to hydroxide ion ? `(` Assume no loss due to evaporation . `)`

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To solve the problem step by step, we will break it down into three parts: identifying the reactions at the anode and cathode, calculating the time required to produce 1 kg of Cl₂, and determining the molarity of the solution with respect to hydroxide ions. ### Step 1: Identify the Reactions at the Anode and Cathode **At the Anode:** The oxidation reaction occurs at the anode where chloride ions (Cl⁻) are oxidized to chlorine gas (Cl₂): \[ 2Cl^-(aq) \rightarrow Cl_2(g) + 2e^- ...
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