Electrochemistry System – code: 7620.01

7620.01
7620.01b

Electrochemistry System 2

Code: 7620.01

Investigating the electrochemical phenomena

Altay’s Electrochemistry System is a powerful instrument to introduce students to the chemical reactions that involve electrical phenomena.

How is electric current produced? Can we store this electric current somehow? Why does iron rust? Is it possible to protect metals from corrosion? Altay’s Electrochemistry System will answer all these questions and many more, through practical demonstrations. The complete set of equipment has been selected to perform the 21 experiments included in the Instruction Manual plus a wide range of additional electrochemistry experiments. The manual helps easily to set up all demonstrations.

Specifications
Size: 77x55x20 cm
Weight: approx. 8.5 kg
Packing: durable aluminium carry case with
foam inserts.

Equipment Suggested
RED pH Meter (code 4840.13)
RED Voltage & Current Sensor (code 4840.16)
Tripod Stand (code 4830.46)

MAIN COMPONENTS

  • Stand with universal clamps
  • Digital multimeter
  • Hand-held pH meter
  • Hoffmann voltmeter
  • DC power supply
  • Long red and black connecting wires
  • Short red and black connecting wires
  • Crocodile clips
  • Iron electrodes
  • Copper electrodes
  • Silver electrodes
  • Zinc electrodes
  • Lead electrodes
  • Aluminium electrodes
  • Platinum electrodes
  • Graphite electrodes
  • 25 ml burette
  • Burette clamp
  • Test cell module
  • Test cell covers
  • Beaker
  • Glass rods
  • Measuring cylinder
  • Glass funnel
  • Bulb lamp set
  • Filter paper

LIST OF EXPERIMENTS

  • Electrolytes and conductivity
  • Conductivity and concentration
  • Electrolytic processes
  • Salt solution cell
  • An unusual source of electric current the lemon cell
  • The standard hydrogen electrode
  • The Daniell cell
  • Connection of Daniell cells
  • The Volta cell
  • Galvanic cells concentration cells
  • Galvanic cells with different redox couple
  • Water electrolysis
  • Water electrolysis basic environment
  • Accumulators
  • The silver /silver chloride reference electrode
  • Standard potentials and the silver/silver chloride reference electrode
  • Plotting a titration curve
  • Weak acid and strong base titration
  • Corrosion and cathodic protection
  • Protection against corrosion: galvanizing
  • Aluminium anodizing

CHEMICAL AND PHYSICAL PROPERTIES

  • Conductivity and electrolytes
  • Effect of concentration on conductivity
  • Dissolution of metals
  • Reference electrodes
  • Reduction potentials
  • Cells
  • Daniell cells
  • Volta cells
  • Concentration cells
  • Connection of cells in series and parallel
  • Practical use of reference electrode:
  • Measuring pH experiments
  • Electrolytic processes
  • Effect of pH on Water electrolysis
  • Corrosion and protection of metals
EXAMPLE OF USE: Water Electrolysis

Demonstrates the composition of water thanks to an electrolytic process.

Water is composed of hydrogen and oxygen in a proportion of 2:1.
The passage of an electric current through a weak acidic or basic water solution causes the decomposition of water into its component gases.
Direct electric current causes the following reactions in the acidified water at the platinum electrodes:
At the cathode (–) 4H++4e– → 2H2
At the anode (+) 6H2O → O2 + 4H3O+ + 4 e–
At the anode, water molecules are oxidised because their electrode potential
( E0 ( O2 / H2O ) = +1.23 V) is lower than that of the sulphate ions SO2-4 ( E0 ( SO2-4 / S2-O2-8 ) = +2.05 V ).
At the cathode, H3O+ ions are reduced because their potential ( E0 ( H+ / H2 ) = + 0 V ) is greater than that of water molecules H2O ( E0 ( H2O / H2 ) = – 0.83 V ).
In the basic environment OH– ions and Na+ ions are present which migrate towards the anode and cathode respectively.
At the cathode, water molecules are reduced because their potential ( E0 ( H2O / H2 ) = – 0.83 V )
is greater than that of the sodium ions ( E0 ( Na / Na+ ) = – 2.73V )
Sodium ions will not undergo any reduction given their very negative reduction potential.
At the anode, OH– ions are oxidised because their potential ( E0 ( O2 / OH– ) = + 0.40 V )
is lower than the potential of the redox couple ( E0 ( O2 /H2O ) = +1.23 V ).
So the reactions will be :
At the cathode (–) 4 H2O + 4e– → 2H2 + 4OH–
At the anode (+) 4OH– → O2 + 2H2O + 4e–
Hydrogen and oxygen collect in the limbs of the Hoffmann Voltameter. The volume occupied by oxygen and hydrogen in the limbs will show the ratio between the two gases. Hydrogen will occupy double the volume of oxygen.

Hoffman apparatus for water electrolysis

P.IVA 12425761009
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