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In an aqueous solution how does specific conductivity of electrolytes change with addition of water?
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pH of solution depends upon concentration of $\mathrm{H}^{+}$present in solution. $\mathrm{pH}$ of the solution will not be affected as $\left[\mathrm{H}^{+}\right]$ remains constant.
At anode : $2 \mathrm{H}_2 \mathrm{O} \longrightarrow \mathrm{O}_2+4 \mathrm{H}^{+}+4 e^{-}$
At cathode : $4 \mathrm{H}^{+}+4 e^{-} \longrightarrow 2 \mathrm{H}_2$
At anode : $2 \mathrm{H}_2 \mathrm{O} \longrightarrow \mathrm{O}_2+4 \mathrm{H}^{+}+4 e^{-}$
At cathode : $4 \mathrm{H}^{+}+4 e^{-} \longrightarrow 2 \mathrm{H}_2$
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