Home
Class 12
CHEMISTRY
The cell Pt|H(2)(g) (1atm)|H^(+), pH = x...

The cell `Pt|H_(2)(g) (1atm)|H^(+), pH = x ||` Normal calomal electrode has EMF of `0.64` volt at `25^(@)C`. The standard reduction potential of normal calomal electrode is `0.28V`. What is the `pH` of solution in anodic compartment. Take `(2.303RT)/(F) = 0.06` at `298K`.

Text Solution

Verified by Experts

`E_(H^(+)//H_(2))^(@) =- 0.06 log.(1)/([H^(+)]) = - 0.06pH`
`rArr 0.64 = E_("cathode") - E_("Anode") = 0.28 -(-0.06pH)`
`rArr pH = (0.64 -0.28)/(0.06) =(0.36)/(0.06) =6`
Promotional Banner

Similar Questions

Explore conceptually related problems

The cell Pt, H_(2) (1atm) H^(+) (pH =x)| Normal calomel Electrode has an EMF of 0.67V at 25^(@)C .Calculate the pH of the solution. The oxidation potential of the calomel electrode on hydrogen scale is -0.28V .

The e.m.f. of the cell obtained by combining Zn and Cu electrode of a Daniel cell with N calomel electrode in two different arrangements are 1.083V and 0.018V respectively at 25^(@)C . If the standard reduction potential of N calomel electrode is 0.28V find the emf og Daniel cell.

The e.m.f. of cell: H_(2)(g) |Buffer| Normal calomal electrode is 0.6885V at 40^(@)C when the barometric pressure is 725mm of Hg. What is the pH of the solution E_("calomal")^(@) = 0.28 .

The EMF of the cell M|M^(n+)(0.02M) ||H^(+)(1M)|H_(2)(g) (1atm)Pt at 25^(@)C is 0.81V . Calculate the valency of the metal if the standard oxidation potential of the metal is 0.76V .

The potential of the following cell is 0.34 volt at 25^@ C. Calculate the standard reduction potential of the Copper half cell. Pt //H_(2 (1 atm )) //H_((1M))^(+) // // Cu_((1m))^(2+) // Cu

The emf of the cell involving the following reaction, 2Ag^(+) +H_(2) rarr 2Ag +2H^(+) is 0.80 volt. The standard oxidation potential of silver electrode is:-

The reduction potential of a half-cell consisting of a Pt electrode immersed in 1.5 M Fe^(2+) and 0.015 M Fe^(3+) solutin at 25^@ C is (E_(Fe^(3+)//Fe^(2+))^@ = 0.770 V) is .