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An excess of Hg was added to 10^(-3) M a...

An excess of Hg was added to `10^(-3) M` acidified solution of `Fe^(3+)` ions. It was found that only `4.6 %` of the ions remained as `Fe^(3+)` at equilibrium at `25^(@)C`. Calculate `E^(@)` for `2Hg//Hg_(2)^(2+)` at `25^(@)C` for
`2Hg+2Fe^(3+) hArr Hg_(2)^(2+)+2Fe^(2+)`

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The correct Answer is:
`-0.7912` volt
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An excess of liquid mercury is added to an acidicfied solution of 1.0xx10^(-3) M Fe^(3+) . It is found that 5% of Fe^(3+) remains at equilibrium at 25^(@)C . Calculate E^(c-)._((Hg_(2)^(2+)|Hg)) assuming that the only reaction that occurs is 2Hg+2Fe^(3+) rarr Hg_(2)^(2+)+2Fe^(2+) Given : E^(c-)._((Fe^(3+)|Fe^(2+)))=0.77V

HgS darr+Na_(2)S hArrNa_(2)[HgS_(2)]

Assertion (A) : Fe^(3+) (g) ion is more stable than Fe^(2+)(g) ion. Reason (R) : Fe^(3+) ion has more number of unpaired electrons than Fe^(2+) ion.

A solution containing SCN^(-) ions can be used to test one or more out of: Fe^(3+),Co^(2+),Cu^(2+),Ag^(+) and Hg^(2+)

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