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Zn(s)+2H^(+)(aq)rarr Zn^(2+)(0.1M)+H(2)(...

`Zn(s)+2H^(+)(aq)rarr Zn^(2+)(0.1M)+H_(2)(g,"1 atm")`
Cell potential of a chemical cell in which the above reaction occurs is `+0.28V` at `25^(@)C`. Write the half-cell reactions and calculate the pH of the hydrogen electrode.
Give : `E_("Zn^(2+)|Zn)^(@)=-0.76V and E_(2H^(+)|H_(2))^(@)=0.00V`.

Text Solution

Verified by Experts

`E_("cell")=E_("cell")^(@)-(0.059)/(2)log.([Zn^(2+)])/([H^(+)]^(2))`
or, `0.28=0.76-(0.059)/(2)log.(0.1)/([H^(+)]^(2))`
or, `16.27=log0.1-2log[H^(+)]" "therefore pH=8.635`
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Zn(s)+2H^(+)(aq)rarr Zn^(2+)(0.1M)+H_(2)(g,"1 atm") Cell potential of a chemical cell in which the above reaction occurs is +0.28V at 25^(@)C . Write the half-cell reactions and calculate the pH of the hydrogen electrode. Give : E_("Zn^(2+)||Zn)^(@)=-0.76V and E_(2H^(+)||H)^(@)=0.00V

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The standard reduction potential of Zn^(2+)|Zn electrode is -0.76 V . What will be the electrode reactions if this electrode is coupled with a standard hydrogen electrode?

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