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. 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

10^{- 25} M

25^{o} C

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

Join BYJU'S Learning Program

By how much is the oxidizing power of Cr2O2−7|Cr3+ couple decreased if the H+ concentration is decreased from 1 M to 10−3M at 25∘C?

The correct option is C 0.414 VHalf cell reaction is Cr2O2−7+14H++6e−→2Cr3++7H2O ECr2O2−7|Cr3+−E∘Cr2O2−7|Cr3+ =−0.0591nlog[Cr3+]2[Cr2O2−7][H+]14 =0.05916log[10−3]14=−0.414V {Option (D)}

By how much is the oxidizing power of $C r_{2} O_{7}^{2 -} | C r^{3 +}$ couple decreased if the $H^{+}$ concentration is decreased from $1 M$ to $10^{- 3} M$ at $25^{\circ} C$ ?