Explain the relation between pH and corrosion of iron Concept introduction: Electro-chemical interaction of metal with the non-metals present in environment resulted in the deformation of the metal surface is called corrosion. Generally they are converted from metal state to oxide, hydroxide or sulfides respectively and found to be more stable than pure metal. In case of uncoated-steel, Fe act as anode and release two and undergoes oxidization to produce Fe 2+ . The half-cell reaction for corrosion can be written as follows. Fe ( s ) → Fe 2+ ( a q ) + 2 e - Generally corrosion was accelerated by warm temperature, water and salts. In addition p H also has strong influence over corrosion. To explain: Influence of p H over the rusting of iron.

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Answer 1

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Chapter 18, Problem 18.64QP

Interpretation Introduction

Interpretation:

Explain the relation between pH and corrosion of iron

Concept introduction:

Electro-chemical interaction of metal with the non-metals present in environment resulted in the deformation of the metal surface is called corrosion. Generally they are converted from metal state to oxide, hydroxide or sulfides respectively and found to be more stable than pure metal. In case of uncoated-steel, Fe act as anode and release two and undergoes oxidization to produce Fe²⁺. The half-cell reaction for corrosion can be written as follows.

Fe(s)→Fe2+(aq) + 2e-

Generally corrosion was accelerated by warm temperature, water and salts. In addition p^H also has strong influence over corrosion.

To explain:

Influence of p^H over the rusting of iron.

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Answer 2

Question

Chapter 18, Problem 18.64QP

Interpretation Introduction

Interpretation:

Explain the relation between pH and corrosion of iron

Concept introduction:

Electro-chemical interaction of metal with the non-metals present in environment resulted in the deformation of the metal surface is called corrosion. Generally they are converted from metal state to oxide, hydroxide or sulfides respectively and found to be more stable than pure metal. In case of uncoated-steel, Fe act as anode and release two and undergoes oxidization to produce Fe²⁺. The half-cell reaction for corrosion can be written as follows.

Fe(s)→Fe2+(aq) + 2e-

Generally corrosion was accelerated by warm temperature, water and salts. In addition p^H also has strong influence over corrosion.

To explain:

Influence of p^H over the rusting of iron.

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Answer 3

Question

Chapter 18, Problem 18.64QP

Interpretation Introduction

Interpretation:

Explain the relation between pH and corrosion of iron

Concept introduction:

Electro-chemical interaction of metal with the non-metals present in environment resulted in the deformation of the metal surface is called corrosion. Generally they are converted from metal state to oxide, hydroxide or sulfides respectively and found to be more stable than pure metal. In case of uncoated-steel, Fe act as anode and release two and undergoes oxidization to produce Fe²⁺. The half-cell reaction for corrosion can be written as follows.

Fe(s)→Fe2+(aq) + 2e-

Generally corrosion was accelerated by warm temperature, water and salts. In addition p^H also has strong influence over corrosion.

To explain:

Influence of p^H over the rusting of iron.

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Answer 4

Question

Chapter 18, Problem 18.64QP

Interpretation Introduction

Interpretation:

Explain the relation between pH and corrosion of iron

Concept introduction:

Electro-chemical interaction of metal with the non-metals present in environment resulted in the deformation of the metal surface is called corrosion. Generally they are converted from metal state to oxide, hydroxide or sulfides respectively and found to be more stable than pure metal. In case of uncoated-steel, Fe act as anode and release two and undergoes oxidization to produce Fe²⁺. The half-cell reaction for corrosion can be written as follows.

Fe(s)→Fe2+(aq) + 2e-

Generally corrosion was accelerated by warm temperature, water and salts. In addition p^H also has strong influence over corrosion.

To explain:

Influence of p^H over the rusting of iron.

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Answer 5

Chapter 18, Problem 18.64QP

Interpretation Introduction

Interpretation:

Explain the relation between pH and corrosion of iron

Concept introduction:

Electro-chemical interaction of metal with the non-metals present in environment resulted in the deformation of the metal surface is called corrosion. Generally they are converted from metal state to oxide, hydroxide or sulfides respectively and found to be more stable than pure metal. In case of uncoated-steel, Fe act as anode and release two and undergoes oxidization to produce Fe²⁺. The half-cell reaction for corrosion can be written as follows.

Fe(s)→Fe2+(aq) + 2e-

Generally corrosion was accelerated by warm temperature, water and salts. In addition p^H also has strong influence over corrosion.

To explain:

Influence of p^H over the rusting of iron.

Answer 6

Chapter 18, Problem 18.64QP

Interpretation Introduction

Interpretation:

Explain the relation between pH and corrosion of iron

Concept introduction:

Electro-chemical interaction of metal with the non-metals present in environment resulted in the deformation of the metal surface is called corrosion. Generally they are converted from metal state to oxide, hydroxide or sulfides respectively and found to be more stable than pure metal. In case of uncoated-steel, Fe act as anode and release two and undergoes oxidization to produce Fe²⁺. The half-cell reaction for corrosion can be written as follows.

Fe(s)→Fe2+(aq) + 2e-

Generally corrosion was accelerated by warm temperature, water and salts. In addition p^H also has strong influence over corrosion.

To explain:

Influence of p^H over the rusting of iron.

Answer 7

Chapter 18, Problem 18.64QP

Interpretation Introduction

Interpretation:

Explain the relation between pH and corrosion of iron

Concept introduction:

Electro-chemical interaction of metal with the non-metals present in environment resulted in the deformation of the metal surface is called corrosion. Generally they are converted from metal state to oxide, hydroxide or sulfides respectively and found to be more stable than pure metal. In case of uncoated-steel, Fe act as anode and release two and undergoes oxidization to produce Fe²⁺. The half-cell reaction for corrosion can be written as follows.

Fe(s)→Fe2+(aq) + 2e-

Generally corrosion was accelerated by warm temperature, water and salts. In addition p^H also has strong influence over corrosion.

To explain:

Influence of p^H over the rusting of iron.

Answer 8

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Answer 9

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Answer 10

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Answer 11

Ch. 18.1 - Permanganate ion and iodide ion react in basic...Ch. 18.1 - Use the half-reaction method to balance the...Ch. 18.1 - Use the half-reaction method to balance the...Ch. 18.1 - Prob. 1PPC Ch. 18.1 - Prob. 18.1.1SR Ch. 18.1 - Prob. 18.1.2SR Ch. 18.3 - A galvanic cell consists of an Mg electrode in a...Ch. 18.3 - Determine the overall cell reaction and Ecell (at...Ch. 18.3 - A galvanic cell with Ecell = 0.30 V can be...Ch. 18.3 - Prob. 2PPC

Solution Summary: The author explains the relationship between pH and corrosion of iron.

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