The magnitude of the change in oxidising power of the $M n O_{4}^{-} / M n^{2 +}$ couple is $x \times 10^{- 4} V$ , if the $H^{+}$ concentration is decreased from $1 M$ to $10^{- 4} M$ at $25 ° C$ . (Assume concentration of $M n O_{4}^{-}$ and $M n^{2 +}$ to be same on change in $H^{+}$ concentration). The value of $x$ is . (Round off to the nearest integer).

[Given: $2.30 R T / F = 0.059$ ]

By how much would the oxidizing power of the $M n O_{4}^{-} / M n^{2 +}$ couple change if the $H^{+}$ ions concentration is decreased to a hundredth of its initial value?

Q. The extent of the oxidising power of (1 M)

M n O_{4}^{-} / M n^{2 +}

(1 M) couple decreased if the

H^{+}

concentration is decreased for 1 M to

10^{- 4}

M at

25^{o}

C is:

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If the H+ concentration is decreased from 1 M to 10−4 M at 25oC for the couple MnO4−/Mn2+, then the oxidising power of the MnO4−/Mn2+ couple decreases by :

The correct option is C 0.38 VInitialE1=Eo−0.05915log[Mn2+](1)8finalE2=Eo−0.05915log[Mn2+](10−4)8E2−E1=0.05915log[Mn2+]×(10−4)8[Mn2+]△E=0.05915log10−32=0.378∼(0.38V)decreases by 0.378VReaction is MnO−4+8H++5e−⟶Mn2++4H2O

If the $H^{+}$ concentration is decreased from $1 M$ to $10^{- 4} M$ at $25^{o} C$ for the couple ${M n O_{4}}^{-} / M n^{2 +}$ , then the oxidising power of the ${M n O_{4}}^{-} / M n^{2 +}$ couple decreases by :