Small pieces of silver, copper, and magnesium are placed in solutions that conta

Question

Small pieces of silver, copper, and magnesium are placed in solutions that contain one of the following ions: Ag^+ Cu^2+ and Mg^2+. The metal/solution combinations tested are summarized in the following table. Any reaction that occurred followed the pattern where M is a general metal and B^+ is a general metal ion. Here is the summary of the observations: In a column, list the oxidizing agents (those being reduced), with the SOA (strongest oxidizing agent) at the top. In a second column, list the reducing agents (those being oxidized), with the SRA (strongest reducing agent) at the bottom. Label the SOA and the SRA.

Explanation / Answer

The more active metal is able to reduce the less active metal cation. This activity series is:

Li>K>Ca>Na>Mg>Al>Zn>Cr>Fe>Ni>Sn>Pb>H2>Cu>Hg>Ag>Pt>Au

            most active                                                                          least active

Here Ag, Cu and Mg are available. According to this series Magnesium metal is able to reduce copper(II) ions and Ag (I) in solution thus Mg is a strong reducing agent agent .

Mg(s)   +   Cu2+(aq)      Mg2+(aq)    +   Cu(s)

Mg(s)   +   2 Ag+(aq)      Mg2+(aq)    +   2Ag(s)

And According to this series Ag is strong oxidizing agent.

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