Activity Series (Reduction Potential)
Introduction
In this experiment you will compare the reactivity of several metals and draw some conclusions as to how this is related to their reduction potential. When one metal is more active than another it will replace the less reactive metal from its compounds. Example:
Zn + Pb(NO3)2 --> Pb + Zn(NO3)2
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Procedure
- Place 10 drops of the zinc nitrate solution in the first well of a 12-well strip. Place 10 drops of the lead nitrate solution in the second well, and 10 drops of silver nitrate solution in the third well. Cut 3 small pieces of copper metal and add one to each of the wells. Allow the strip to stand at least 5 minutes while you observe and record any reactions. (Continue with the remaining procedures while these mixtures stand.)
- Well 1:
- Well 2:
- Well 3:
- Skip one well and place 10 drops of copper nitrate in well 5, 10 drops of lead nitrate in well 6, and 10 drops of magnesium nitrate in well 7. Add a small piece of shiny zinc metal to each well. Observe and record the results.
- Well 5:
- Well 6:
- Well 7:
- In wells 9, 10, and 11, repeat the procedure using the zinc, lead and potassium nitrate solutions with small pieces of magnesium metal. Record your results.
- Well 9:
- Well 10:
- Well 11:
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Questions
- Write balanced equations for all the reactions which were observed in the above procedures.
- Make a list of the metals used to run this experiment in order of decreasing activity. Remember, one metal is more active than another if it will replace that metal from its compounds.
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Safety
Wear eye protection at all times. Several of the compounds are toxic. Do not ingest the chemicals. Wash your hands before leaving the laboratory.
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TG Materials
- The following solutions stored in pipet storage devices:
- 0.1 M Zn(NO3)2 (dissolve 3.0 g Zn(NO3)2•6H2O in enough distilled water to make 100 mL of solution)
- 0.1 M Cu(NO3)2 (dissolve 2.3 g Cu(NO3)2•2.5H2O in enough distilled water to make 100 mL of solution)
- 0.1 M KNO3 (dissolve 1.0 g KNO3 in enough distilled water to make 100 mL of solution)
- 0.1 M Mg(NO3)2 (dissolve 2.6 g Mg(NO3)2•6H2O in enough distilled water to make 100 mL of solution)
- 0.1 M Pb(NO3)2 (dissolve 3.3 g Pb(NO3)2 in enough distilled water to make 100 mL of solution)
- 0.1 M AgNO3 (dissolve 1.7 g AgNO3 in enough distilled water to make 100 mL of solution)
- The following metals stored in microcentrifuge tubes:
- magnesium metal
- zinc metal
- copper metal
- 12-well strip
- cotton swabs
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