SOME INVESTIGATIONS ON THE CORROSION OF IRON
Mayceemae M. Barnuevo
CHEM 17.1 13L
Group 1
February 7, 2014
February 19, 2014
Exercise 12
SOME INVESTIGATIONS ON THE CORROSION OF IRON
I.
Introduction
Metals undergo natural destruction that allows a spontaneous deteriorating reaction where they return to their original state from where they are obtained upon contact with the surrounding, particularly when reacted to oxygen. Such phenomenon is known as corrosion (Zumdahl, 1998). This leads the surface of the materials to rust in due time. Usually, this kind of process is electrochemical but is sometimes accompanied by mechanical and physical stress that causes the metal to corrode (Heitz et al, 1992).
Iron, a common type of metal in the form of alloy steel which is widely used in construction firms, gradually corrodes upon being oxidized into ions of irons by oxygen and forms rust as a result of electrochemical reaction. In addition, at room temperature, pH, presence of water and electrolytes would also contribute to the formation of rust on its surface (Wilbraham et al, 2003).
The objective of this exercise is to state the effects of the following factors on the corrosion of iron:
1. acidity and basicity of the solution in contact with the metal;
2. mechanical stress applied on the metal; and
3. contact with other metals.
1
II.
Materials
A. Reagents
0.1 M potassium ferricyanide, K3Fe(CN)6 ferrous sulphate, FeSO4 sodium hydroxide, NaOH sodium chloride, NaCl hydrochloric acid, HCl potassium hydroxide, KOH potassium nitrate, KNO3 nitric acid, HNO3 trisodium phosphate, Na3PO4 sodium thiocyanate, NaSCN sulfuric acid, H2SO4 distilled water, dH2O
B. Apparatus test tubes
iron ring
250-mL beaker
iron stand
bunsen burner
C. Others iron nails
copper strip
sand paper
zinc strip
pliers
2
III.
Procedure
A. Reactions of Iron with various Aqueous Solutions
In determining the reactions of iron immersed in various aqueous
solutions, three set-ups were made, each consists of four test tubes with iron
nails
CHEM 17.1 13L
Group 1
February 7, 2014
February 19, 2014
Exercise 12
SOME INVESTIGATIONS ON THE CORROSION OF IRON
I.
Introduction
Metals undergo natural destruction that allows a spontaneous deteriorating reaction where they return to their original state from where they are obtained upon contact with the surrounding, particularly when reacted to oxygen. Such phenomenon is known as corrosion (Zumdahl, 1998). This leads the surface of the materials to rust in due time. Usually, this kind of process is electrochemical but is sometimes accompanied by mechanical and physical stress that causes the metal to corrode (Heitz et al, 1992).
Iron, a common type of metal in the form of alloy steel which is widely used in construction firms, gradually corrodes upon being oxidized into ions of irons by oxygen and forms rust as a result of electrochemical reaction. In addition, at room temperature, pH, presence of water and electrolytes would also contribute to the formation of rust on its surface (Wilbraham et al, 2003).
The objective of this exercise is to state the effects of the following factors on the corrosion of iron:
1. acidity and basicity of the solution in contact with the metal;
2. mechanical stress applied on the metal; and
3. contact with other metals.
1
II.
Materials
A. Reagents
0.1 M potassium ferricyanide, K3Fe(CN)6 ferrous sulphate, FeSO4 sodium hydroxide, NaOH sodium chloride, NaCl hydrochloric acid, HCl potassium hydroxide, KOH potassium nitrate, KNO3 nitric acid, HNO3 trisodium phosphate, Na3PO4 sodium thiocyanate, NaSCN sulfuric acid, H2SO4 distilled water, dH2O
B. Apparatus test tubes
iron ring
250-mL beaker
iron stand
bunsen burner
C. Others iron nails
copper strip
sand paper
zinc strip
pliers
2
III.
Procedure
A. Reactions of Iron with various Aqueous Solutions
In determining the reactions of iron immersed in various aqueous
solutions, three set-ups were made, each consists of four test tubes with iron
nails
Bibliography: Heitz, E., Henkhaus, R., Rahmel, A. 1992. Corrosion. In Academic American Encyclopedia. Petrucci, R. H., Herring, F. G., Madura, J. D., and Bissonnette, C. 2011. Silberberg, M. S. 2013. Principles of General Chemistry. 3rd ed. New York, NY. Wilbraham, A. C., Staley, D. D, Matta, M. S. and Waterman, E. L. 2003. Whitten, K. W., Davis, R. E., Peck, M. L., Stanley, G. G. 2010. Chemistry. 9th 12 Zumdahl, S. S. 1998. Chemical Principle. 3rd ed. Boston. Houghton Company