Zinc Metal Ions

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How does a variation in the concentration of metal ions of the cathode in a Zinc-Copper electrochemical cell affect the electrical potential?
Introduction:

In a highly technological and quickly developing society, it is imperative to innovation that basic components are understood and explored to further expansion and advancement. In order to understand how everyday necessities such as cars, computers, and cell phones are constantly powered, it must first be understood what is in a battery as well as what happens to the ions within the battery. This can be explained by electrochemistry and the reaction that occurs within a battery, which is induced and explored in this experiment. The reaction that occurs within a battery cell is an oxidation-reduction
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This hypothesis is supported by the redox reaction that will take place and the cell potential, ECell, which measures the potential difference between two half cells in an electrochemical cell . During the redox reaction, when one substance is oxidized and loses electrons, it becomes positively charged, or becomes the anode . In this experiment, the anode is the Zinc metal in the Zinc solution. Conversely, during reduction the substance gains electrons and become negatively charged, and becomes the cathode , and in this experiment the cathode is the Copper metal in the Copper solution. Thus, during the experiment the Zinc half-cell will be losing electrons as the Copper half-cell will gain more electrons, and since the Copper half-cell is increased, there will be greater concentrations of Copper ions than Zinc ions . The hypothesis can also be further supported when examining the equation to determine the voltage or cell potential between the two electrodes, E_Cell=E_Cathode-E_Anode. From the equation, it can be summarized that since the difference between the anode’s potential to become oxidized and the cathode’s potential to become reduced is calculated, when increasing the concentration of metal ions in the cathode, the potential will also be increased, as thus the difference …show more content…
Fill two 80mL beakers with 60mL of accurately measured water. Set up measuring scale and make sure the unit is on grams. Place 1 measuring boat onto scale and zero the scale. Using a scoopula, gently place small scoops of Zinc Chloride onto the measuring boat until reaching the desired amount of 1.5g. This should be the controlled amount fo Zinc Chloride throughout the experiment. Remember to carefully place the material onto the measuring boat for maximum accuracy. When desired grams of Zinc Chloride is obtained, take the boat off the scale and dump contents into one of the 80mL beakers with water. Place Zinc metal strip into the beaker and stir the solid content well for 10 seconds or when it has clearly dissolved. Attach one end of black wire onto the 1 lead and the other end onto the top of the Zinc material. Repeat steps 7-9 with Copper Chloride and the Copper metal piece. Attach one end of the red wire onto the 5 lead and the other end onto the top of the copper material. Rip a thin strip of paper from a paper towel and dip said strip into the Potassium Nitrate solution until the strip is fully

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