Metal Potentials Experiment

[cs_content][cs_section parallax=”false” separator_top_type=”none” separator_top_height=”50px” separator_top_angle_point=”50″ separator_bottom_type=”none” separator_bottom_height=”50px” separator_bottom_angle_point=”50″ style=”margin: 0px;padding: 45px 0px;”][cs_row inner_container=”true” marginless_columns=”false” style=”margin: 0px auto;padding: 0px;”][cs_column fade=”false” fade_animation=”in” fade_animation_offset=”45px” fade_duration=”750″ type=”1/1″ style=”padding: 0px;”][cs_text]Production of Materials‎ > ‎4. Electrochemical Methods‎ >

Perform a first-hand investigation and gather first-hand information to measure the difference in potential of different combinations of metals in an electrolyte solution[/cs_text][/cs_column][/cs_row][/cs_section][cs_section parallax=”false” separator_top_type=”none” separator_top_height=”50px” separator_top_angle_point=”50″ separator_bottom_type=”none” separator_bottom_height=”50px” separator_bottom_angle_point=”50″ style=”margin: 0px;padding: 45px 0px;”][cs_row inner_container=”true” marginless_columns=”false” style=”margin: 0px auto;padding: 0px;”][cs_column fade=”false” fade_animation=”in” fade_animation_offset=”45px” fade_duration=”750″ type=”1/1″ style=”padding: 0px;”][cs_text]

  • The difference in potential of different combinations of metals in electrolyte solutions can be measured using the following procedure:
    • Select two metals (Metal A and Metal B) and arrange them and their solutions as shown below:

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Experimental setup

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    • Observe and record the reading given by the voltmeter.
    • If the voltmeter gives a reading of zero, reverse the terminals, and observe and record the reading again.
    • If the voltmeter gave a positive reading with the initial terminal arrangement, then Metal B is the more easily oxidised metal, while Metal A is the more easily reduced metal.
    • If the voltmeter gave a positive reading after the terminals were reversed, then the nature of the metals is the opposite to the above.
    • The voltage reading corresponds to the difference in potential of the two metals.
    • Repeat the above procedure with different metals in place of Metal B.
    • Use Metal A as a standard (allocate it a potential of zero) to create a table of approximate reduction potentials using the results obtained.
  • In reality, the standard hydrogen electrode is the chosen reference electrode, and is allocated a potential of zero.
  • The standard hydrogen electrode consists of:
    • Platinum foil coated in fine platinum powder dipping into a solution containing 1 mol. L-1 hydrogen ions.
    • Hydrogen gas of 100 kPa pressure and 25°C temperature bubbling over the electrode.
  • When the standard hydrogen half-cell forms one half of a galvanic cell with another half-cell, then the potential difference of the whole cell is a measure of the standard electrode potential of the second half-cell.

 


Example setup using copper and zinc

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