Determine the oxidizing strengths of metal ions Cu2+, Zn2+, Mg2+, Ag+
The reduction potentials (how likley they are to REDUCE)
Cu2+ + 2 e− is in equilibrium with Cu(s) +0.337
Zn2+ + 2 e− is in equilibrium with Zn(s) −0.7618
Mg2+ + 2 e− is in equilibrium with Mg(s) −2.372
Ag+ + e− is in equilibrium with Ag(s) +0.7996
then, if we want the OXIDATION strneght, we must invert every set
Cu(s) is in equilibrium with Cu2+ + 2 e− -0.337
Zn(s)is in equilibrium with Zn2+ + 2 e− +0.7618
Mg(s) is in equilibrium with Mg2+ + 2 e− +2.372
Ag(s) is in equilibrium with Ag+ + e− -0.7996
the most easy to oxidize will be Mg
the least will be AG
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