The observed emf of the cell, `Pt|H_(2) ("1 atm")|H^(+)(3xx10^(-4) M)||H^(+) (M_(1))|H_(2) ("1 atm")|Pt` is 0.154 V. Calculate the value of `M_(1)` and pH of cathodic solution.

The observed emf of the cell, `Pt|H_(2) ("1 atm")|H^(+)(3xx10^(-4) M)|

1.	The observed emf of the cell, `Pt\|H_(2) ("1 atm")\|H^(+)(3xx10^(-4) M)\|\|H^(+) (M_(1))\|H_(2) ("1 atm")\|Pt` is 0.154 V. Calculate the value of `M_(1)` and pH of cathodic solution.
Answer» `E_(cell)=0.0591" log" M_(1)/(3xx10^(-4))` or `"log"M_(1)/(3xx10^(-4))=0.154/0.0591=2.6058` `M_(1)/(3xx10^(-4))=4.034xx10^(2)` `M_(1)=4.034xx10^(2)xx3xx10^(-4)M` `=0.121 M` `pH=-log[H^(+)]=-log 0.121=0.917`

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The observed emf of the cell, `Pt|H_(2) ("1 atm")|H^(+)(3xx10^(-4) M)||H^(+) (M_(1))|H_(2) ("1 atm")|Pt` is 0.154 V. Calculate the value of `M_(1)` and pH of cathodic solution.

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