Experiment_607_Single Displacement Reactions_1_1_1

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Student Name

Laboratory Date:

Date Report Submitted:

___________________________

Student ID

Experiment Number and Title

Experiment 607: Single Displacement Reactions

Experiment 607: Single Displacement Reactions

Section 1: Purpose and Summary

Carry out single displacement reactions involving (a) metals with salts of other metals, and (b) metals with dilute acid.
Determine the order of activity of metals and hydrogen based on observations.

Note: ‘Single displacement reactions’ are sometimes called ‘single replacement reactions’.

In this experiment, students will conduct different reactions between a metal and a salt of another metal. Students will also conduct reactions between metals and dilute acid solution. Based on observations, students will list the metals and hydrogen in order of activity.

Section 2: Safety Precautions and Waste Disposal

Safety Precautions:

Use of eye protection is recommended for all experimental procedures.

Waste Disposal:

While you are doing the experiment, pour your liquid waste into a beaker. Separate the solid metal pieces from the waste solution.

Metal pieces should be rinsed with water, and then they may be disposed of in proper solid waste container.

When you are finished with the experiment, collect the liquids into a waste beaker (liquid waste only). Transfer the liquid waste into the inorganic waste container in the fume hood.

Section 3: Procedure

Some combinations of reactants used in this experiment may react slowly or be difficult to detect at times. If you see no immediate visible result, set the test tube aside and allow it to stand for 5 to 10 minutes, then reexamine it.

To determine whether a reaction occurs or not, observe any bubble formation (gas evolution) in the solution or a change in appearance of the metallic solid (note the color and/or texture).

Part 1: Reaction of metal with aqueous metal salt solution

Obtain four (4) pieces each of magnesium, copper, zinc, and iron metals. If necessary, clean the metal piece with fine sandpaper or steel wool until the surface is clean and shiny. Surface coatings on these metals may inhibit chemical reactions.

Rinse three (3) test tubes with laboratory water and shake out the excess water. Label them with Cu, Zn, and Fe. Set them up in your test tube rack.

In each of the test tubes, place about 1 mL (20 drops) of magnesium nitrate solution. Add a piece of metal (except for magnesium metal) to each test tube. Observe the metal pieces for evidence of reaction. Note, if any, change in the color of the solution. Record your observations in the table below. If no change is observed, write ‘no reaction’.

Repeat steps 2 and 3, using a different metal salt solution and set of metals.

	with Mg(NO₃)₂(aq)
Cu(s)
Zn(s)
Fe(s)

	with Cu(NO₃)₂(aq)
Mg(s)
Zn(s)
Fe(s)

	with Zn(NO₃)₂(aq)
Mg(s)
Cu(s)
Fe(s)

	with Fe(NO₃)₃(aq)
Mg(s)
Cu(s)
Zn(s)

Part 2: Reaction of metal with dilute acid solution

Rinse four (4) test tubes with laboratory water and shake out the excess water. Label them with Mg, Cu, Zn, and Fe. Set them up in your test tube rack.

In each of the test tubes, place about 1 mL (20 drops) of hydrochloric acid solution. Add a piece of metal to each test tube. Observe the metal pieces and the solution for evidence of reaction. Record your observations in the table below. If no change is observed, write ‘no reaction’.

	with HCl(aq)
Mg(s)
Cu(s)
Zn(s)
Fe(s)

Post-lab Questions:

Write balanced molecular equation, complete ionic equation and net ionic equation for each reaction that you observed in this experiment.

Based on your observations, list Mg, Cu, Zn, Fe, and H in order of increasing activity (least to highest).

Aluminum lies below magnesium and above zinc in the reactivity series of metals. Predict its reaction with each of the metal solutions and dilute acid solution used in this experiment.