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The emf of the cell : H(2)(g)|"Buffer||N...

The emf of the cell : `H_(2)(g)|"Buffer||Normal"` canlomel elctrolde is `0.6885V` at `25^(@)C`, when barometric pressure is `=760 mm`. What is the pH of the buffer solution? `E_("calomel")=0.28V`

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The e.m.f of the cell : H_2(g) |Buffer | Normal calomel electrodes is 0.6885 volt at 25^(@)C , when barometric pressure is 760 mm Hg. What is the pH of the buffer solution ? Given E_("calomel")^(@) = 0.28 volt

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 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 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 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 .

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 .

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 .

The EMF of the cell : Pt|Ce^(4+)(90%),Ce^(3+)(10%)| Normal calomel electrode is 1.464 V at 25^(@)C . Find the value of equilibrium constant of the reaction : 2Ce^(3+)+2H^(o+) rarr 2Ce^(4+)+H_(2) The electrode potential of the normal calomel electrode is +0.28V .

The EMF of the cell : Pt|Ce^(4+)(90%),Ce^(3+)(10%)| Normal calomel electrode is 1.464 V at 25^(@)C . Find the value of equilibrium constant of the reaction : 2Ce^(3+)+2H^(o+) rarr 2Ce^(4+)+H_(2) The electrode potential of the normal calomel electrode is +0.28V .