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Cathodic Protection 1.0 Introduction

Cathodic protection (CP) is a technique used to control the corrosion of a metal surface by making it the cathode of an electrochemical cell. A simple method of protection connects the metal to be protected to a more easily corroded "sacrificial metal" to act as the anode.Common applications are fuel pipelines, steel water pipelines etc.

2.0 Objectives.

The students are able to understand the concept of cathodic protection by i. Sacrificial anode. ii. Impressed current

3.0 Theory

In a galvanic series for a particular medium, metals which have more positive electrode potentials will act as cathodes while those which have less positive or more negative potentials will become anodes. Table 6.1 shows a galvanic series of metals and alloys in seawater.
In order to protect a metal from corrosion, it should be coupled with another metal of more negative electrode potential. The metal which acts as an anode will corrode. This method is called corrosion protection by sacrificial anode. A metal might be also protected by forcing the electrode potential to be more positive to become cathode. It is achieved by supplying cathodic current to the metal. This method also known as cathodic protection by impressed current.

4.0 Materials and Apparatus.

1. DC voltmeter and ammeter 2. Salt solution, 3% NaCl (30g NaCl in 1000ml solution) 3. Salt solution, 1% NaCl (10g NaCl in 1000ml solution) 4. 0.5N H2SO4 5. Two 250ml beakers 6. Zinc, steel, aluminium and platinum plates. 7. One saturated calomel electrode (SCE) 8. A rheostat 9. A 12 DC power supply.

5.0 Experiment Method

6.1 Corrosion protection by sacrificial anode.

a) The beaker was filled with 200ml of 3% NaCl solution. b) A steel plate was immersed into the solution and was connected to SCE as shown on Figure 6.1 c) The electrode potential of the connection was measured. d) Now the steel was replaced with zinc and again, the connection potential was recorded. e) The steps above in 4.1(d ) was repeated for aluminium plate. f) Steel and aluminium plates was connected to a voltmeter and an ammeter as illustrated in Figure 6.2 and immersed in 3% NaCl Solution and the reading was recorded. g) Step 4.1(f) was repeated by replacing aluminium with zinc plate. h) Steps 4.1(a) to 4.1(g) were repeated by using 1% NaCl solution i) Steps 4.1(a) to 4.1(g) were repaeated again using 0.5N H2SO4 j) The results were formed in tabulation form.

6.2 Corrosion Protection by Impressed Current

a) A beaker was filled with 200ml of 3% NaCl solution. b) Both steel and platinum plates was connected to power supply, ammeter voltmeter, and a rheostat as shown in Figure 6.3 c) The rheostat was adjusted to appropriate positions and the reading was recorded from voltmeter and ammeter readings. d) Steps 4.2(a) to 4.2(c) was repeated for 15 NaCl then for 0.5N H2SO4

6.0 Tabulation of Data. 7.0 4.1)Corrosion protection by sacrificial anode.

3% NaCl solution | Electrode Potential (V) | | 1 | 2 | 3 | Average | Steel & SCE | 0.940 | 0.954 | 0.962 | 0.952 | Zinc & SCE | 0.867 | 0.870 | 0.875 | 0.871 | Aluminium & SCE | 0.732 | 0.736 | 0.730 | 0.733 | 3% NaCl solution | Voltmeter Readings (mV) | Ammeter Readings (mA) | | 1 | 2 | 3 | Average | 1 | 2 | 3 | Average | Steel & Aluminium | 44.40 | 67.10 | 62.40 | 57.97 | 0.52 | 0.26 | 0.33 | 0.37 | Steel & Zinc | 13.40 | 32.50 | 58.50 | 34.80 | 1.89 | 1.03 | 1.84 | 1.59 |

1% NaCl solution | Electrode Potential (V) | | 1 | 2 | 3 | Average | Steel & SCE | 215.6 | 216.8 | 211.5 | 214.63 | Zinc & SCE | 0.925 | 0.895 | 0.906 | 0.909 | Aluminium & SCE | 0.724 | 0.701 | 0.677 | 0.701 | 1% NaCl solution | Voltmeter Readings (mV) | Ammeter Readings (mA) | | 1 | 2 | 3 | Average | 1 | 2 | 3 | Average | Steel & Aluminium | 20.6 | 14.7 | 96.2 | 43.83 | 0.21 | 0.35 | 0.21 | 0.26 | Steel & Zinc | 135.7 | 58.9 | 127.6 | 107.4 | 0.62 | 0.76 | 0.74 | 0.71 |

0.5N H2SO4 solution | Electrode Potential (V) | | 1 | 2 | 3 | Average | Steel & SCE | 157.3 | 174.8 | 161.5 | 164.53 | Aluminium & SCE | 0.719 | 0.644 | 0.581 | 0.648 | Zinc & SCE | 0.889 | 0.898 | 0.892 | 0.893 |

0.5N H2SO4 solution | Voltmeter Readings (mV) | Ammeter Readings (mA) | | 1 | 2 | 3 | Average | 1 | 2 | 3 | Average | Steel & Aluminium | 24.9 | 25.9 | 20.4 | 23.73 | 1.33 | 1.40 | 1.41 | 1.38 | Steel & Zinc | 0.03 | 0.05 | 0.04 | 0.04 | 0.09 | 0.09 | 0.07 | 0.08 |

4.2 Corrosion Protection by Impressed Current
3% NaCl solution Position of Rheostat | Voltmeter Readings (V) | Ammeter Readings (mA) | | 1 | 2 | 3 | Average | 1 | 2 | 3 | Average | 1 | 15.8 | 12.6 | 11.56 | 13.32 | 0.82 | 0.61 | 0.13 | 0.52 | 2 | 10.6 | 4.6 | 4.4 | 6.53 | 0..18 | 0.18 | 0.09 | 0.15 | 3 | 0.883 | 0.862 | 0.743 | 0.829 | 1.80 | 0.38 | 1.41 | 1.20 |

0.5N H2SO4 solution Position of Rheostat | Voltmeter Readings (V) | Ammeter Readings (mA) | | 1 | 2 | 3 | Average | 1 | 2 | 3 | Average | 1 | 22.9 | 17.9 | 9.7 | 16.83 | 1.09 | 0.81 | 0.14 | 0.68 | 2 | 41.6 | 16.4 | 20.9 | 26.3 | 1.51 | 0.57 | 0.88 | 0.99 | 3 | 0.893 | 0.844 | 0.835 | 0.857 | 0.38 | 0.63 | 0.76 | 0.59 |

1% NaCl solution Position of Rheostat | Voltmeter Readings (V) | Ammeter Readings (A) | | 1 | 2 | 3 | Average | 1 | 2 | 3 | Average | 1 | 11.05 | 11.57 | 11.04 | 11.22 | 0.46 | 0.30 | 0.44 | 0.40 | 2 | 6.39 | 6.44 | 9.87 | 7.57 | 0.22 | 0.20 | 0.20 | 0.21 | 3 | 20.49 | 20.9 | 16.9 | 19.43 | 0.11 | 0.12 | 0.10 | 0.11 |

8.0 Discussions a) Discuss the effect of type of ions and their concentration on corrosion rate of a sacrificial anode.

The different types of ion involve in this process affect the rate of ion discharging . The more electronegative of the ion involved , the higher the rate of ion discharging aand the corrosion rate of sacrificial anode.
The concentration of ions also affect the corrosion rate.The higher the concentration of the solution involved, the higher of potential value and the higher the rate of corrosion. Based on the Nernst Equation as shown below: E= E + RT/ZF ln [ion]

where [ion] is the concentration of ions in the solutions. From the equation above we know that, the potential is directly proportional to the concentration of ion.

b) Explain the ability of aluminium in protecting steel compare to zinc.

Based on electrochemical series, the electrode potential of aluminium is -1.66V while for zinc is –0.76V.So, aluminium is more electronegative than zinc. The electronegativity of aluminium will form oxide layer that can protect and prevent corrosion on the steel and also stopping the oxidation process from occurs. Therefore aluminium is better than zinc as to protect steel from corrosion.

c) Describe the advantages and disadvantages of the cathodic protection methods by sacrificial anode and impressed current. | Advantages | Disadvantages | Impressed Current | * No need to replace the protection plate. * unlimited current opportunities and longer life | * Needs power supply. * Expansive to set up. * Higher levels of current | Sacrificial Anode | * sacrificial anode can be replace once unusable. * Power supply is not needed * Cheaper | * Difficult to apply extra protection towards metal. * Sacrificial anode have to be changed frequently * Not practical for large scale installation where long-term corrosion protection is required. |

In this experiment , the aluminium plate should have the higher reading of voltmeter and ammeter than zinc and steel since aluminium more electronegative han other. There was systematics error which the voltmeter and ammeter didn’t work very well and also the connection of the circuit may not connected very well and tight.

9.0 Precaution

* Make sure the connection is well connected and tight. * Be sure to rub off the plate before doing the experiments. * Make sure once both plates are immersed into the solution, the plates must not touch to each other.

10.0 Conclusion.

From the experiments , we can conclude that there two types of way to prevent the corrosion to happen in the steel. By using sacrificial anode way where the metal that used to be corroded rather than the other metals that want to be protected or using Impressed current method, power supply is used in order to prevent the metal we want to protect is not undergoes corrosion.

11.0 Appendix Voltmeter
V
V

Metal Beaker Electrolyte SCE

Figure 6.1

V
V

A
A

Metal Beaker Electrolyte Metal (Al)

Figure 6.2

Power supply

A
A

Rheostat
V
V Metal Beaker Electrolyte Pt

Figure 6.3

12.0 Referrences.

1. Subbarao,E.C., Chakravorty , D., Merrican, M.F. and Raghevan, V.,1972. Experiments in Materials Science. New York: McGraw Hill.
2. Jones, D.A., 1996. Principles and Prevention of Corrosion, 2nd Edition, Upper Saddle, New Jersey :Prentice Hall.
3. The Science and Engeneering of Materials, 11th Edition. Donald R. Askeland and Predeep P.Pule. Topic 20-Corrosion and Degradation

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