The significant difference between the ionization constant values of [ F e ( H 2 O ) 6 ] 3 + and [ F e ( H 2 O ) 6 ] 2 + has to be explained. Concept introduction: Hydrated transition metal ions are weak acids. There are M − O − H bonds in the hydrated metal ions. Transition metal ions have large charges and small sizes to attract the shared pair of the M − O bonds to the metal ion itself. This attraction weakens the O − H bond making the hydrogen of the M − O − H bond more acidic than it would be in the O − H bond of a water molecule that is not bonded to a metal ion. Thus, hydrated transition metal ions can donate proton and the solution becomes acidic.

Question

Want to see the full answer?

Answer 1

Question

Chapter 14, Problem 75QRT

Interpretation Introduction

Interpretation:

The significant difference between the ionization constant values of [Fe(H2O)6]3+ and [Fe(H2O)6]2+ has to be explained.

Concept introduction:

Hydrated transition metal ions are weak acids. There are M−O−H bonds in the hydrated metal ions. Transition metal ions have large charges and small sizes to attract the shared pair of the M−O bonds to the metal ion itself.

This attraction weakens the O−H bond making the hydrogen of the M−O−H bond more acidic than it would be in the O−H bond of a water molecule that is not bonded to a metal ion. Thus, hydrated transition metal ions can donate proton and the solution becomes acidic.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Students have asked these similar questions

Write a complete balanced net ionic equation where Cr(NO3)3 added to NaOH in aqueous solution results in Cr(OH)4-

All the following salts are alkaline except LiClO NH4NO3 SrCrO4 K2HPO4

Is the interaction between an ammonia ligand and a metal cation a Lewis acid-base interaction?

Answer 2

Question

Chapter 14, Problem 75QRT

Interpretation Introduction

Interpretation:

The significant difference between the ionization constant values of [Fe(H2O)6]3+ and [Fe(H2O)6]2+ has to be explained.

Concept introduction:

Hydrated transition metal ions are weak acids. There are M−O−H bonds in the hydrated metal ions. Transition metal ions have large charges and small sizes to attract the shared pair of the M−O bonds to the metal ion itself.

This attraction weakens the O−H bond making the hydrogen of the M−O−H bond more acidic than it would be in the O−H bond of a water molecule that is not bonded to a metal ion. Thus, hydrated transition metal ions can donate proton and the solution becomes acidic.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 3

Question

Chapter 14, Problem 75QRT

Interpretation Introduction

Interpretation:

The significant difference between the ionization constant values of [Fe(H2O)6]3+ and [Fe(H2O)6]2+ has to be explained.

Concept introduction:

Hydrated transition metal ions are weak acids. There are M−O−H bonds in the hydrated metal ions. Transition metal ions have large charges and small sizes to attract the shared pair of the M−O bonds to the metal ion itself.

This attraction weakens the O−H bond making the hydrogen of the M−O−H bond more acidic than it would be in the O−H bond of a water molecule that is not bonded to a metal ion. Thus, hydrated transition metal ions can donate proton and the solution becomes acidic.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 4

Question

Chapter 14, Problem 75QRT

Interpretation Introduction

Interpretation:

The significant difference between the ionization constant values of [Fe(H2O)6]3+ and [Fe(H2O)6]2+ has to be explained.

Concept introduction:

Hydrated transition metal ions are weak acids. There are M−O−H bonds in the hydrated metal ions. Transition metal ions have large charges and small sizes to attract the shared pair of the M−O bonds to the metal ion itself.

This attraction weakens the O−H bond making the hydrogen of the M−O−H bond more acidic than it would be in the O−H bond of a water molecule that is not bonded to a metal ion. Thus, hydrated transition metal ions can donate proton and the solution becomes acidic.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 5

Chapter 14, Problem 75QRT

Interpretation Introduction

Interpretation:

The significant difference between the ionization constant values of [Fe(H2O)6]3+ and [Fe(H2O)6]2+ has to be explained.

Concept introduction:

Hydrated transition metal ions are weak acids. There are M−O−H bonds in the hydrated metal ions. Transition metal ions have large charges and small sizes to attract the shared pair of the M−O bonds to the metal ion itself.

This attraction weakens the O−H bond making the hydrogen of the M−O−H bond more acidic than it would be in the O−H bond of a water molecule that is not bonded to a metal ion. Thus, hydrated transition metal ions can donate proton and the solution becomes acidic.

Answer 6

Chapter 14, Problem 75QRT

Interpretation Introduction

Interpretation:

The significant difference between the ionization constant values of [Fe(H2O)6]3+ and [Fe(H2O)6]2+ has to be explained.

Concept introduction:

Hydrated transition metal ions are weak acids. There are M−O−H bonds in the hydrated metal ions. Transition metal ions have large charges and small sizes to attract the shared pair of the M−O bonds to the metal ion itself.

This attraction weakens the O−H bond making the hydrogen of the M−O−H bond more acidic than it would be in the O−H bond of a water molecule that is not bonded to a metal ion. Thus, hydrated transition metal ions can donate proton and the solution becomes acidic.

Answer 7

Chapter 14, Problem 75QRT

Interpretation Introduction

Interpretation:

The significant difference between the ionization constant values of [Fe(H2O)6]3+ and [Fe(H2O)6]2+ has to be explained.

Concept introduction:

Hydrated transition metal ions are weak acids. There are M−O−H bonds in the hydrated metal ions. Transition metal ions have large charges and small sizes to attract the shared pair of the M−O bonds to the metal ion itself.

This attraction weakens the O−H bond making the hydrogen of the M−O−H bond more acidic than it would be in the O−H bond of a water molecule that is not bonded to a metal ion. Thus, hydrated transition metal ions can donate proton and the solution becomes acidic.

Answer 8

Expert Solution & Answer

Answer 9

Expert Solution & Answer

Answer 10

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 11

Ch. 14.1 - Identify each molecule or ion as a Brnsted-Lowry...Ch. 14.1 - Using Le Chatelier’s Principle Use Le Chatelier’s...Ch. 14.1 - Prob. 14.3E Ch. 14.1 - Complete the table. Ch. 14.1 - Prob. 14.4E Ch. 14.1 - Prob. 14.5E Ch. 14.2 - Prob. 14.6CE Ch. 14.2 - Prob. 14.7E Ch. 14.3 - Prob. 14.2PSP Ch. 14.3 - Prob. 14.3PSP

Solution Summary: The author analyzes the difference between the ionization constant values of left[Fe (H_2O)6 right]3+ and

Videos

Want to see the full answer?

Chapter 14 Solutions

Solution Summary: The author analyzes the difference between the ionization constant values of left[Fe (H_2O)­6 right]3+ and

Videos

Want to see the full answer?

Chapter 14 Solutions

Solution Summary: The author analyzes the difference between the ionization constant values of left[Fe (H_2O)6 right]3+ and