Link to Penny Chemistry, part 1

Last time, we used a mixture of salt and vinegar to remove the tarnish from pennies. This time, we will get back some of the dissolved copper by collecting it on some iron nails. To try this you will need:

• a small glass, cup, or bowl
• vinegar
• salt
• several pennies
• several iron nails

The start of this experiment is pretty much a repeat of part of last week's experiment. Put a couple of inches of vinegar into a cup. Add a teaspoon of salt, and give it a stir to help it dissolve. This time, instead of dipping a penny halfway into the solution, drop in several pennies.

Very quickly, you will see the same thing happen that we saw last time. The pennies will lose their coating of oxides, becoming bright and shiny. In the process, some of the copper is being dissolved in the vinegar/salt solution.

To get some of that copper back, drop a couple of iron nails into the solution. After a minute or so, you will see tiny bubbles forming on the nails. After an hour or so, look at the nails again. They should have a thin coating of copper.

Why does the copper coat the nails? The solution that dissolved the copper from the pennies is also dissolving some of the iron from the nails. As the atoms of iron dissolve, they leave behind electrons, giving the nail a negative electric charge. Both the iron and copper atoms dissolved in the solution have a positive charge, but the copper is more strongly attracted to the nail, so the copper atoms stick to it, forming a coating.

The bubbles are hydrogen gas, produced by a reaction between the hydrogen ions from the vinegar and the metals. Once enough copper atoms have been deposited to balance out the negative charge on the nail, the process stops.

Does it make a difference if the nail is touching the penny? Try suspending the nail by a string, so it does not touch the copper. Does it still work? To see a stronger contrast, try suspending the nail so that only half is in the vinegar. That part should get a copper coating, while the part above the liquid should remain as it is.

Way back in the 70's, when I was working at the Memphis Pink Palace Museum, part of our Kitchen Chemistry program involved using packets of ketchup to remove the tarnish from pennies. You take a dull, brown, tarnished penny and rub it with some ketchup. In seconds, the penny is bright and shiny. Usually, the experiment stops there, but I thought we might take a look to see why it works. To try this, you will need:

• ketchup
• water
• vinegar
• salt
• potassium chloride (salt substitute)
• 5 small cups or bowls
• 6 or more tarnished pennies
• labels and a marker

Safety Warning

Before you go wild with pouring different chemicals together, remember to keep safety in mind. For the stuff in your refrigerator and spice cabinet, you can pretty much mix whatever you want. Tuna fish and grape jelly may not be tasty, but it will not explode or burn off your fingers. Outside your refrigerator, you need to be much more careful. Cleaning supplies and other household chemicals can be harmful by themselves, and if the wrong ones are mixed they can be deadly. Only use them for experiments that specifically call for them.

Experiment

A good place to start is with the original experiment. Put a little ketchup onto one of the tarnished pennies. Let is sit there for about 30 seconds, and then rinse it. What you should find is that the tarnish has been removed from the part of the penny that was in the ketchup. OK, so that works just as well as it did back in the 70's.

Next, take a look at the ingredients for the ketchup. Besides tomatoes, you will notice that two prominent chemicals are vinegar and salt. A little internet research will show you many other science experiments that use vinegar and salt for doing the same thing as the ketchup. If you want to be sure that the tomatoes are not responsible for cleaning the pennies, try using some tomato sauce that does not contain vinegar or salt.

After some experimentation, you will probably find that the vinegar and salt are the important ingredients but are they both necessary? Lets find out. Start with four small cups. Put about an inch of water in one. That will be our control. The control does not contain any of the chemicals that we are testing. If it cleans the pennies too that would tell us that the reaction happens, even without the vinegar or salt. Label this cup "Control."

In the second cup, put about an inch of vinegar. Label this one "Vinegar."

In the third cup, put about an inch of water, and then add a teaspoon of salt. Give it a quick stir to dissolve the salt. Label this one "Salt Water."

In the fourth cup, put about an inch of vinegar, and add a teaspoon of salt. Give it a quick stir to dissolve the salt. Label this cup "Vinegar and Salt."

Now, you are ready to do some testing. Lets start with the Control. Dip one of the tarnished pennies halfway into the water, and hold it there for 30 seconds. Remove it from the water, rinse it, and put it beside the Control cup.

Do the same for each of the other cups. Be sure to give each 30 seconds, and be sure to rinse the penny to remove any vinegar or salt. Place each penny beside the solution you used to test it.

Results

OK, now what did you find? If your results were like mine, you found that neither the water, the vinegar, or the salt water did much, if anything to the pennies. The mixture of salt and vinegar was very effective at removing the tarnish.

So what is happening? The tarnish on the penny is copper oxide, and a chemical reaction with the vinegar will actually dissolve it. Then why did the pure vinegar not work? With the penny and the vinegar, you get a series of chemical reactions that form a circle. One reaction removes the copper, but just as quickly, another reaction puts it back. In chemistry, this is known as an equilibrium reaction.

The trick is to add something that will interrupt that equilibrium. You want a chemical that will grab the copper before it can be put back, and the table salt does a very good job of that.

What is it about the table salt that grabs the copper? Table salt is sodium chloride. When you put it in water, it separates into sodium ions (charged atoms) and chlorine ions, but is it the sodium or the chlorine that grabs the copper. An easy way to test that is with a different kind of salt. One of the common salt substitutes is potassium chloride. You can find it beside the regular (sodium chloride) salt at the grocery. In a fifth cup, put about an inch of vinegar and stir in a teaspoon of potassium chloride. Does it work the same as the table salt? If so, then it is the chlorine that grabs the copper. If not, then it is either the sodium, or the combination of sodium and chlorine.

You can look deeper into the vinegar as well. Will it work with other acids? Try using lemon juice (citric acid and ascorbic acid) or carbonated drinks (carbonic acid). Carbonated colas also contain phosphoric acid. Again, remember safety. Look for acids from your refrigerator and spice cabinet, not from other household chemicals.

Link to Penny Chemistry, part 2

This week's experiment comes from Burning Questions, my program on the science of fire. When teaching about fire, educators frequently talk about the fire triangle to teach about how things burn. Just as a triangle has to have three sides to be a triangle, you need three things to have a fire: Fuel, heat, and oxygen. Recently, fire educators have started teaching about the fire diamond instead of the fire triangle, because sometimes having fuel, heat and oxygen is not enough to get a fire. To see this, you will need:

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Two weeks ago, I mentioned that I had a lot of fun experimenting with carbonated soda (and drinking it) and that I should do an experiment with chocolate. I got quite a few e-mails suggesting experiments with chocolate, but this one was the most common. It has to do with the white discoloration that you sometimes find on old chocolate. For this week's experiment, you will need:

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This week's experiment came from a shopping trip. I recently paid for my groceries with a $50 bill. Most stores test large bills with a special pen, to see if they are counterfeit, but this store had run out of the special pens. Instead, they put a drop of iodine on the bill to be sure that it was good. To see why, you will need:

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A few weeks ago, we looked at a classic experiment of putting a lit candle under a glass. We saw that water was drawn into the glass, not by the oxygen being burned up, but by the cooling of the air in the glass after the candle went out. This experiment will allow us to do what many people thought the first experiment was doing, measure the amount of oxygen in the air.

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This week's experiment is a fun one and a yummy one too. (I was hungry while I was choosing it.) We are going to experiment with the impact that vitamin C has on the browning of fruit.

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A simple experiment to show how photographs work.

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It is amazing how many books get this one wrong!

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Instant Fizz

What is the difference between baking soda and baking powder? And why should you care?

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What is Smoke?

We frequently see smoke, but what is it made of?

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Cleaning the Silver

A little kitchen chemistry can make a difficult job quick and easy.

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Pictures in Silver

Use chemistry to produce an image on a piece of silverware.

A fun but smelly test to find tannins in your food.

This project has Science Fair potential.

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Two weeks ago, we took the first steps in learning about how soap was once made by using water to dissolve potassium hydroxide out of paper ashes. You can find part one at: http://thehappyscientist.com/science-experiment/wood-ash

If we had been serious about making soap, we would have used a lot more ashes, probably from a wood fire. We would have dissolved the potassium hydroxide in water and then would have boiled the water to concentrate the chemicals.

Once we had a strong solution, we would have mixed the strong base with fat or oil for a process called saponification. The result would have been soap.

This week, we will do something very similar, on a much smaller scale. To try this, you will need:

- a dirty sink
- a sponge
- a porcelain cleaner that contains bleach. I used a product called Soft Scrub with bleach and it worked very well. Comet Cleanser with bleach also worked very well.

First, be careful. Anything that contains bleach can leave white, bleached spots on clothing, and can irritate your eyes.

Wet the sponge and the sink. Apply the cleaner with the sponge. Be sure to follow the directions on the package, and use it properly. Then scrub the sink. Do a good job, and get all the corners.

When you are done, rinse the sink well. While your fingers are wet, rub them together. They should feel very slippery. That slippery feeling is the result of saponification. The bleach in the cleaner is sodium hypochlorite, a strong base, just as potassium hydroxide is. A strong base will react with the fatty acids in the fat to produce soap and glycerol.

Soap? Did we really just make soap? Yes that slippery feeling is the result of saponification of the oils in your skin. The same basic process is used in oven cleaners and chemicals to open clogged drains. A strong base will convert the grease in the oven or drain into soap, which can be washed away.

Now, to make any of that into a really nice, useable soap, it would take more processing to balance the fat with the basic chemical, and then remove the impurities. Still, you really did make a tiny bit of soap. I do not recommend the process for cleaning your hands, but you are sure to get compliments on the nice, clean sink. If you want to experiment more, I am sure that the tub could use cleaning too. You might even earn a nice bowl of ice cream.

Have a wonder-filled week.