How to Make Oxygen and Hydrogen from Water Using Electrolysis

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Two Parts:Setting up the EquipmentConducting Your ExperimentCommunity Q&A

The process of splitting water (H₂O) into its atomic components (hydrogen and oxygen) using electricity is known as electrolysis. This experiment has significant implications in terms of what these 2 gases can be used for in their own right, with hydrogen being one of the cleanest sources of energy we have access to. Although it may sound complicated, it's actually easier than you think if you have the right equipment, the right knowledge, and a little bit of know-how.

Steps

Part 1

Setting up the Equipment

1. 1

   Fill a 350 ml (12  fl oz) glass with warm water.

   You don’t need to fill it all the way to the top, so leave a little bit of room. If the water is warm, it will conduct the electricity more effectively but it will also still work just fine with cold water.

   ^[1]

   • You can use either water from out of the tap or bottled water, it doesn't matter which.
   • Warmer water has a lower viscosity and allows ions that conduct electricity to move more freely.

2. 2

   Dissolve 1 tbsp (17 g) of table salt in your water.

   All you need to do is pour it in and then stir it around a little bit to help it dissolve. This turns it into a saline solution.

   ^[2]

   • Sodium chloride (which is table salt) is an electrolyte which helps aid the conductivity of the water, as water by itself isn’t particularly conductive.
   • By making the water more conductive, the current from the battery flows through more easily which results in the water being split into hydrogen and oxygen more effectively.

3. 3

   Sharpen both ends of 2 #2 pencils so the graphite is exposed.

   Make sure to remove the eraser at the top of the pencil. You need to sharpen the pencils enough that the graphite is fully exposed at both ends.

   ^[3]

   • These graphite shafts that are encased within the pencil are your electrodes and will conduct the electricity that comes from the battery.
   • The graphite works really well as it doesn’t dissolve or get damaged in the water while you conduct the experiment.

4. 4

   Cut a square piece of cardboard that is big enough to cover the glass.

   Use cardboard that is thick enough to maintain its structural integrity when it has some holes punched through it. Try cutting a square portion out of a shoebox or some other kind of thick box.

   ^[4]

   • The purpose of the cardboard is to suspend the pencil graphite in the water without allowing it to touch the walls of the glass.
   • Because cardboard has no metallic properties to it, it can sit on top of your glass without affecting the outcome of the experiment.

5. 5

   Punch 2 holes in the cardboard using the 2 pencils.

   Use the actual pencils to do this as you need to snugly fit the pencils into the holes so the pencils don't move around or slip. If the graphite touches the walls or the base of the glass, it will interrupt the experiment.

   ^[5]

Part 2

Conducting Your Experiment

1. 1

   Connect one end of each alligator clip to the terminals of the battery.

   The battery is what actually produces the electrical current and so the alligator clips provide the pathway for transporting that current to the water. You need to attach one clip to the positive terminal and one to the negative terminal.

   ^[6]

   • Use a 6-volt battery but if you cannot find one, use a 9-volt battery.
   • You can find this size of battery at pretty much any convenience store or supermarket.

2. 2

   Connect the other end of each alligator clip to each pencil.

   Make sure that the metallic part of the alligator clip is connected to the graphite of the pencil. You may have to shave down a little bit more of the wood from the pencil just to make sure that the alligator clips are completely connected to the graphite.

   ^[7]

   • Doing this completes the connection to the battery and allows the current to be transferred from the battery all the way through into the water.

3. 3

   Place the cardboard on top of the glass so the pencils are submerged.

   The way you cut the cardboard earlier means that it should sit nicely on top of the glass. Try to do this gently so that the pencils that are stuck through the cardboard don’t get disturbed from their position.

   ^[8]

   • For this experiment to work, the graphite of the pencils needs to not be touching the side of the glass so just double check that here and adjust the pencils if need be.

4. 4

   Watch the separation of hydrogen and oxygen occur.

   At this point, bubbles start to rise from the submerged points of graphite. This is the hydrogen and oxygen gas being split. Hydrogen gas will be bubbling from the pencil connected to the negative terminal and oxygen will be bubbling from the pencil connected to the positive terminal.

   ^[9]

   • Once you connect the alligator clips to the battery and graphite, the current begins to flow immediately.
   • There will be more bubbles coming from the hydrogen pencil because there is twice as much hydrogen as oxygen in each water molecule.

Community Q&A

Add New Question

• Question

  How do I store hydrogen gas separately?

  wikiHow Contributor

  Community Answer

  Hydrogen is less dense than oxygen so it should rise to the top of the container, though you would not be able to see it. With this in mind, theoretically if you used a bottle rather than a cup and had a small tube to run the hydrogen off with you could potentially store the hydrogen separately. Though hydrogen is highly flammable/can be explosive, so it's not recommended to store in large quantities. If you want to start getting technical, there are also sensors you can buy that recognize the presence of O2 and H2, which you could use in addition to small pumps so you could separate the hydrogen made and use it as a fuel source.

• Question

  Is this activity safe for sixth grade?

  It all depends on the safety precautions taken during the experiment. Hydrogen is easily flammable and requires oxygen to burn. Before presenting the experiment in front of the class, make sure you understand the process. Safety equipment like as goggles and gloves are recommended.

• Question

  Would it be safe to breathe in chloride?

  wikiHow Contributor

  Community Answer

  No. Chloride is an extremely dangerous gas, and should not be inhaled under any circumstances. Fortunately, there will only be a tiny bit of chloride present in this experiment and should not cause you much harm--unless you use a very high voltage battery. Nonetheless, it would be a good idea to avoid inhaling any chloride gases, regardless of the amount.

• Question

  Is this activity safe for kids around 5th grade?

  wikiHow Contributor

  Community Answer

  Hydrogen gas is extremely flammable and will burn whenever oxygen is introduced so if you do this, make sure an competent adult who understands the process is included.

• Question

  I've tried this but no effects are noticeable. I have added salt and checked the battery for power. How can I fix this?

  wikiHow Contributor

  Community Answer

  You could try moving the electrodes closer together. If they are far away then electricity won't conduct. Also, you can try using baking soda instead of salt.

• Question

  How can I store my separate oxygen?

  wikiHow Contributor

  Community Answer

  You won't be able to store the oxygen you produce from this method due to the temperature.

• Question

  How do I filter off oxygen from the chloride gas?

  wikiHow Contributor

  Community Answer

  You can't.

• Question

  Will this activity be dangerous for a fourth grade science project?

  wikiHow Contributor

  Community Answer

  Yes! It is dangerous because hydrogen is highly flammable and O2 will only feed the flame.

• Question

  If Hydrogen is oxidized will it ignite?

  Hydrogen will not ignite when it's combined with oxygen. However, oxygen will feed the flame.

• Question

  What does 4e- and 4H+ mean in the reaction 2 H2O > 4e- + 4H+ + O2?

  wikiHow Contributor

  Community Answer

  4e- is the transfer of electrons and the 4H+ shows that the hydrogen has an overall positive charge from losing its electrons. The process can be predicted from the periodic table. Hydrogen has a lower electron affinity, so it will lose its electrons before oxygen. Affinity moves from left to right and bottom to top. Flourine has the highest affinity. The electric current is the energy that frees the electrons, breaking the bond between Hydrogen and the Oxygen.

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Tips

• If you can’t find graphite pencils, you can use little pieces of wire instead and just wrap them around the battery on one end, and leave the other end in the water. This has the same effect as the pencils.
• Try using a different sized battery. This will affect the size of the current that goes through the water which will, in turn, affect the speed at which the water molecules get split.

Warnings

• Do this experiment under the supervision of an adult as you are working with electricity and gases which, although unlikely, do have the potential to be harmful.
• Once you add an electrolyte like salt to increase the conductivity, just be aware that there is a small amount of chlorine by-product that gets created. This isn’t enough to be dangerous, but you may notice a subtle smell of chlorine.

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