The Effect Of Electrochemical Cells On Sodium Sulfate Solutions

The purpose of this experiment is to study what happens when you split water molecules using electricity. The hydrogen gas produced can be used as renewable fuel and help slow down global warming, and conserve natural resources. During the process, an electric current from the battery will be transferred to a sodium sulfate solution and change the pH at each electrode. There will be three sub-experiments with 10 trials each to analyze the variables in the experiment including a 9-volt potential, 18-volt potential, and a sodium hydroxide solution. The pH will be measured two ways, through litmus testing paper and litmus indicator-(phenolphthalein). The independent variables will be the applied voltage and starting pH whilst the dependent variable is the pH and amount of gas produced. To ensure that there are no differences that can affect the results, the controlled variable(s) will include the sodium sulfate solution, electrodes such as nailsl, and the 9-volt battery. Considering that pH is the measure of hydrogen and hydroxyl ions, the hypothesis is that during electrolysis, pH rises at the cathode, where hydroxyl ions are synthesized, and declines at the anode, where hydrogen ions are developed. Collectively, the 18-volt battery produces almost twice as much hydrogen gas as when you use a 9-volt and produces a faster reaction. Further on, if the starting solution is made basic by adding sodium hydroxide, then there was little change of the pH observed on the cathode due to the strong alkaline solution.