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Abstract

Objective

Experiment with the effect of pH on the corrosion of copper using a test solution that contains a chemical that turns deep blue in the presence of copper.

Introduction

Copper is an essential element for all known living organisms, including humans. You need a small amount of copper in your diet to stay healthy. On average, most people will eat and drink about 1,000 a (µg) of copper per day—drinking water normally contributes approximately 150 micrograms per day. Levels of copper found naturally in ground water and surface water are typically very low—about 4 µg of copper in one liter (L) of water or less—however, drinking water may contain higher levels of copper, usually as a result of flowing through copper pipes. High levels of copper can occur if water that is corrosive comes in contact with copper plumbing and copper-containing fixtures. Many factors can make water corrosive for copper pipes: low pH (acidic water), dissolved salts and minerals, bacteria, and suspended solids, such as sand, sediment, and rust. The level of copper in drinking water increases with the corrosivity of the water and the length of time it remains in contact with the plumbing. If the copper level gets too high, the water may have a metallic taste and you might notice blue or blue-green stains around sinks and plumbing fixtures. It will be highest in the morning because the water will have been exposed to the pipes overnight. If you are being served by a public water system, the owner of the utility will have results of copper sampling, which is a process that has been done in parts of the water-distribution system.

In this chemistry science fair project, you will demonstrate how the pH of water affects the rate at which copper dissolves. To learn more about pH, you can check out the Science Buddies Acids, Bases, and the pH Scale guide. You will test the theory that acidic water is more corrosive for copper pipes than non-acidic water. In the procedure, copper pennies will be placed in either plain water or in water with acetic acid (vinegar). You will see the progress of the reaction by watching the pennies go from dull and dingy to bright and shiny. The pennies get shiny because copper oxide is being removed by the action of the acid, which results in increasing levels of copper in the liquid. Unfortunately, water that is acidic, or corrosive for other reasons, eats away at the pure copper, as well as at the copper oxide. For houses with corrosive water systems, this can result in elevated levels of copper in the drinking water. On a purely practical level, houses with corrosive water systems might find that their copper pipes are springing leaks, and that the whole house needs to be re-piped with plastic pipes!

To measure the amount of copper present in the solutions that are used to clean the pennies, you will perform a color-based chemical test. The chemicals for the test are contained in a small tablet, which is dissolved in water. When the tablet is dissolved, the solution turns red. If no copper (or very small amounts of copper) is present, the solution remains red. If copper is present, the solution will turn blue. There are additional tests in the kit for pH, iron, and calcium, which you can also use for other experiments, but this science fair project focuses on the copper test. If you are interested in trying this chemistry science fair project, search your house or your parents' car for some old pennies and let's get started!

Terms, Concepts, and Questions to Start Background Research

• Copper
• Element
• Corrosive
• Acid
• pH
• Acetic acid
• Control solution

Questions

• What is the concentration of copper in your tap water, according to the government organization that supplies your drinking water? They test for copper and many other water contaminants to make sure the water supply is safe.
• What does the pH scale measure?
• Based on your research, what are some ways your body uses copper?
• Based on your research, what are some negative consequences of having too much copper in your water supply?

Bibliography

• Winter, M. (2009). Copper. Retrieved October 24, 2009, from http://www.webelements.com/copper/
• Wikipedia Contributors. (2009, October 26). Copper. Wikipedia: The Free Encyclopedia. Retrieved October 24, 2009, from http://en.wikipedia.org/w/index.php?title=Copper&oldid=322183844
• Wisconsin Department of Natural Resources. (2003). Copper and Your Health. Retrieved October 25, 2009, from http://www.dnr.state.wi.us/org/water/dwg/copper.htm

Materials and Equipment

• Copper/Iron Test Kit. The kit contains copper test tablets in a blister pack (10). You can order the kit online from www.thesciencefair.com, item # LM5877.
• Test tubes, size 16mm x 150mm, available from online suppliers like www.thesciencefair.com, item # 6135-5-012
• Graduated cylinder, 10mL volume, available from online suppliers like www.thesciencefair.com, item # 5250-1
• Distilled water; available at most grocery stores (1 gallon)
• Skewers, bamboo or metal, for mixing
• Vinegar, white
• Permanent marker
• Lab notebook
• Plastic cups, 16-ounce (oz.) size (12)
• Pennies, should all be dull and dingy (30)
• Note: Pennies made before 1982 were 95% copper, whereas pennies made after 1982 are mostly zinc with a thin copper plating. Both kinds will work in this procedure.
• Timer or stopwatch
• Strainer with a handle, small
• Paper towels
• Liquid measuring cup, metric
• Optional: Additional copper TesTabs. You can either order a second Copper/Iron Test Kit, or order tablets directly from the manufacturer, LaMotte Company, at www.lamotte.com.
• The procedure below can be done without ordering additional tablets, but it is highly recommended that you obtain additional tablets to allow for extra trials and further experimentation.
• Optional: Chemical safety goggles

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Experimental Procedure

Important Note Before You Begin: The procedure below is designed for students who have not yet had a chemistry class in school. It can be modified to provide more-accurate readings of the copper concentration by using more-advanced test kits, if desired. See the Variations section, below, for sources of more-advanced chemistry kits.

Creating the Control Solutions

1. Using the graduated cylinder, fill one of the test tubes with 10 milliliters (mL) of distilled water.
2. Fill another test tube to 10 mL with vinegar.
3. Add a copper test tablet to each tube, following the directions in the kit.
4. Using skewers, mix the contents in the test tubes until the tablets disintegrate and fall apart.
5. Make a note of the colors of the solutions in your lab notebook.
1. These are control solutions that show the baseline color—meaning, without exposure to copper.

Placing the Pennies in the Water and Vinegar Solutions.

1. Label four of the plastic cups, as follows:
1. Water 1
2. Water 2
3. Vinegar 1
4. Vinegar 2
2. Using the liquid measuring cup, pour 100 mL of vinegar in the cup labeled Vinegar 1.
3. Pour 100 mL of distilled water in the cup labeled Water 1.
4. Drop five pennies into each cup.
1. Note: The kit suggests adding salt, but leave it out for this procedure. Vinegar contains acetic acid, which makes the reaction proceed faster.
5. Start the timer. Wait for 10 minutes.
6. Remove the pennies from the cups, using the strainer, as follows.
1. Pour the contents of the Water 1 cup into the Water 2 cup, catching the pennies with the strainer.
2. Rinse the pennies with tap water and place them on some dry paper towels. Make sure you keep track of from which cup they came.
3. Pour the contents of the Vinegar 1 cup into the Vinegar 2 cup, catching the pennies with the strainer.
4. Rinse the pennies with tap water and place them on some dry paper towels, again keeping track of from which cup they came.

Testing the Solutions for Copper

1. Using the graduated cylinder, fill a clean test tube to 10 mL with the water from the cup labeled Water 2 (which was originally the water from the Water 1 cup).
   1. Always rinse and dry the graduated cylinder between uses.
2. Fill another test tube to 10 mL with vinegar from the cup labeled Vinegar 2 (which was originally the vinegar from the Vinegar 1 cup).
3. Add one copper test tablet to each test tube.
4. Use the skewers to mix the contents of the test tubes until the tablets disintegrate and fall apart.
   1. The solution will turn blue if copper is present (or brown if a small amount of copper is present).
5. Hold the test tube against the white part of the Copper Color Chart that is supplied with the kit.
6. Match the color of the solution to the color on the chart.
7. Record the results in your lab notebook.

Cleaning the Test Tubes and Repeating the Tests

1. Pour out the contents of the two test tubes from the cups with pennies into a sink.
2. Wash the solutions down the drain with running water.
3. Rinse out the test tubes with water.
4. Place them upside down on paper towels.
5. Carry out the procedure two more times, as follows. This will demonstrate that your results are repeatable.
1. Start with the Placing the Pennies in the Water and Vinegar Solutions section.
2. Do not repeat the controls.
3. Use fresh pennies and cups.
6. When the procedure is complete, rinse out the test tubes that contained the samples and the controls and allow them to dry on paper towels.
7. Make a data table showing the color of the water and vinegar test solutions for each trial.
8. What do your results tell you about how pH affects the corrosion of copper pipes?

Troubleshooting

For troubleshooting tips, please read our FAQ for From Dull to Dazzling.

Variations

• Measure the concentration of copper in the solutions using a test kit that provides more-accurate readouts for copper concentration, such as the Hach Copper Color Cube Kit, item# 21822-00, 0-2.5 mg/L Cu. Visit www.hach.com to find where you can buy this kit.
• Devise a procedure to determine how the rate of copper corrosion varies with the pH of the water.
• Test the copper concentration in the drinking water at your home using a copper test kit. Compare the levels in the morning vs. later in the day after the system has been flushed out.
• Devise a procedure for testing how salt (sodium chloride) affects the rate of corrosion of copper pipes.

• For more science project ideas in this area of science, see Chemistry Project Ideas.

Credits

David B. Whyte, PhD, Science Buddies

Last edit date: 2012-01-24 09:00:00