Practical activity Electrolysis There are a number of ways that you could carry out electrolysis in Chemistry. This is an outline of the required steps to undertake one of these methods. Aims To investigate the electrolysis of copper II sulfate solution, and of sodium chloride solution, using inert unreactive electrodes. Place two graphite rods into the copper sulfate solution.
Add about 2 heaped spatulas of sodium chloride. Then add several drops of Universal Indicator solution. Stir to mix thoroughly. You need enough indicator to give the water a reasonable depth of green colour. This is most easily done using electrode holders.
A piece of white paper held behind the U-tube can help. Make sure the U-tube is kept very still during the experiment. This will probably take less than 5 minutes. Teaching notes This experiment is an interesting introduction to the electrolysis of brine. It is probably best not used as the first electrolysis that students encounter.
They would really struggle to explain for themselves what is going on. It could be followed by the electrolysis of salt solution in industry. Students should be able to notice bubbles of gas at each electrode.
At the positive electrode, the indicator turns red initially, and is then bleached to colourless. This indicates the presence of chlorine. At the negative electrode the indicator turns purple.
The remainder of the solution stays green. The product at the negative electrode is hydrogen. This can be difficult for students to understand. When the sodium chloride is dissolved in water, the ions forming the ionic solid separate out.
This means that there are actually 4 ions present in the solution: The negative ions are attracted to the positive electrode. The chloride ions are discharged giving chlorine in preference to the hydroxide ions. These are left behind in solution. At the negative electrode, the hydrogen ions are discharged producing hydrogen gas in preference to the sodium ions.
These are also left behind in solution. Thus sodium hydroxide solution remains. This is the cause of the purple colour of the indicator at the negative electrode.
In time, the green colour of the indicator in the middle would change too, as the ions diffuse through the resulting solution. Students use Universal Indicator to help them follow what is happening during the reaction.
This collection of over practical activities demonstrates a wide range of chemical concepts and processes. Each activity contains comprehensive information for teachers and technicians, including full technical notes and step-by-step procedures.To investigate the electrolysis of copper(II) sulfate solution, and of sodium chloride solution, using inert.
electrodes. Method Core practical for inert electrodes. An Analysis of the Experiment, Electrolysis of Sodium Solution for Gases. 1, words. 5 pages. An Analysis of the Experiment, Energy Produced of Different Alcohols. 2, words.
15 pages. An Analysis of What Factors Affect the Energy Conversion in a . Electrolysis of Sodium Chloride Solution Cautious electrolysis of NaCl solution with the Brownlee apparatus will produce hydrogen plus aqueous NaOCl if the experiment is carried out in a single, unpartitioned jar with stirring.
SODIUM CHLORATE is an odorless pale yellow to white crystalline solid.
It is appreciably soluble in water and heavier, so may be expected to sink and dissolve at a rapid rate. Although it is not itself flammable, the solid product and even 30% solutions in water are powerful oxidizing agents.
Contact with wood, organic matter, ammonium salts, sulfur, sulfuric acid, various metals, and other. Electrolysis of Copper(II) Sulphate Solution Experiment 1 Aim: To investigate the electrolysis of copper(II) sulphate solution and dilute sulphuric acid.
Materials: mol dm -3 copper(II) sulphate solution, mol dm -3 sulphuric acid and wooden splint. Oct 02, · In the water-baking soda solution, the gases that are produced are hydrogen (H 2), oxygen (O 2) and carbon dioxide (CO 2).
Table salt, or sodium chloride (NaCl), is also a good additive to form electrolytes.4/5(K).