Consider the following aqueous ions of first-row transition elements: Mn³⁺, Co³⁺, Ti²⁺, V²⁺, Cr²⁺ (a) Using the standard reduction potential (at 298 K, acidic medium), identify which of the given ions

Question

Consider the following aqueous ions of first-row transition elements:

Mn³⁺, Co³⁺, Ti²⁺, V²⁺, Cr²⁺

(a) Using the standard reduction potential (at 298 K, acidic medium),

identify which of the given ions are thermodynamically strong oxidizing agents in acidic solution. Denote their number as X.

(b) For the given determine which species behave as strong reducing agents. Capable of liberating $H_{2}$ gas from dilute $H^{+}$ . Denote their number as Y.

Hence, compute $\frac{3 X}{Y}$ .

TestHub · Accepted Answer

The correct answer is 2.00

From NCERT D Block

An examination of the $E^{-}$ values for the redox couple $M^{3 +} / M^{2 +}$ show that $Mn^{3 +}$ and $Co^{3 +}$ ions are the strongest oxidising agents in aqueous solutions. The ions $Ti^{2 +}, V^{2 +}$ and $Cr^{2 +}$ are strong reducing agents and will liberate hydrogen from dilute acid, e.g., $2 Cr^{2 +} (aq) + 2 H^{+} (aq) \to 2 Cr^{3 +} (aq) + H_{2} (g)$

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