Examine the following half-reactions and select the strongest reducing agent among the species listed: hgo(s) + h2o(l) + 2e– hg(l) + 2oh–(aq) e°= 0.0977 v zn(oh)2(s) + 2e– zn(s) + 2oh–(aq) e°= –1.25 v ag2o(s) + h2o(l) + 2e– ag(s) + 2oh–(aq) e°= 0.342 v b(oh)3(aq) + 7h+(aq) + 8e– bh4–(aq) + 3h2o(l) e°= –0.481 v

Zn(OH)2(s) + 2e– Zn(s) + 2OH–(aq) E°= –1.25 V

Explanation:

The best reducing agent must have the most negative reduction potential. According to iupac convention, the reduction potential is used to depict the standard redox potentials of substances. Reducing agents have very negative reduction potentials while oxidizing agents have more positive reduction potentials.