(A) Use data from Tables 19.1 and 23.4 to determine whether nitric acid can be used to oxidize V³⁺(aq) to VO²⁺(aq) for standard-state conditions. If so, write a balanced equation for the reaction.

(B) Select a reducing agent from Table 19.1 that can be used to reduce VO²⁺(aq) to V²⁺(aq) for standard-state conditions in acidic solution. Consider that the reduction occurs in two stages: VO²⁺(aq) → V³⁺(aq) → V²⁺(aq), but note that the V²⁺(aq) must not be reduced to V(s).

Tables 19.1

Tables 23.4

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TABLE 19.1 Standard Reduction Potentials at 298.15 K and 1 atma Reduction Half-Cell Reaction Acidic solution F₂(g) + 2 e 2 F (aq) O3(g) + 2 H+ (aq) + 2 e O₂(g) + H₂O(1) S₂O² (aq) + 2 e 2 SO4²(aq) H,Oz(aq) + 2H*(aq) +2e <2H,O(1) Ce+ (aq) + e Ce³+ (aq) MnO₂ (aq) + 4H*(aq) + 3 e¯ ⇒ MnO₂(s) + 2 H₂O(1) PbO₂(s) + SO² (aq) + 4H* (aq) + 2e Cl₂(g) + 2 e 2 Cl(aq) Cr₂O7² (aq) + 14 H*(aq) + 6 e¯ — 2 Cr³+ (aq) + 7 H₂O(1) MnO2 (s) + 4H+ (aq) + 2 e Mn²+ (aq) + 2 H₂O(1) O₂(g) + 4H+(aq) + 4e 2 H₂O(1) IO3 (aq) + 12 H¹ (aq) + 10 e Br₂(1) 2 e 2 Br NO3(aq) + 4H(aq) + 3 e¯¯ — NO(g) + 2 H₂O(1) Ag¹(aq) + e Ag(s) Zn(s) Al(s) = Mg(s) Fe³+ (aq) + e Fe²+ (aq) Oz(g) +2H*(aq) +2e