Which metals may be oxidized by h+ under standard-state conditions? ag+(aq) + e– → ag(s) e° = 0.80 v cu2+(aq) + 2e– → cu(s) e° = 0.34 v sn2+(aq) + 2e– → sn(s) e° = –0.14 v zn2+(aq) + 2e– → zn(s) e° = –0.76 v

Answer is: tin and zinc, because they standard potential as less than zero.
Tin and zinc are oxidized to tin and zinc cations (with +2 charge) and hydrogen anions are reduced to hydrogen molecules with neutral charge.
Zn → Zn²⁺ + 2e⁻; 2H⁺ + 2e⁻ → H₂.
Oxidation is increase of oxidation number  and reduction is decrease of oxidation number.

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