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. If the

H^{+}

concentration 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

Q. By how much would the oxidising power of the

(M n O_{4}^{-} | M n^{2 +})

couple change if the

H^{+}

ions concentration is decreased

100

times at

25^{\circ} C

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By how much is the oxidizing power of MnO−4/Mn2+ electrode changes when concentration of H+ ion decreases from 1 M to 10−25 M at 25oC?

The correct option is A 2.36VIn Acidic medium, MnO−4+8H++5e−→Mn2++4H2O[H+]=1 M⇒E1=EoMnO−4/Mn2+−0.0595 log[Mn2+][MnO−4][1]8[H+]=10−25 ME1−E2=0.0595 log1[10]8=0.0595×200=2.36 V∴ Oxidizing power of MnO−4/Mn2+ decreases by 2.36 V

By how much is the oxidizing power of $M n O_{4}^{-} / M n^{2 +}$ electrode changes when concentration of $H^{+}$ ion decreases from $1 M$ to $10^{- 25} M$ at $25^{o} C$ ?