   Chapter 14, Problem 157AE

Chapter
Section
Textbook Problem

# The equilibrium constant Ka for the reaction Fe ( H 2 O ) 6 3+ ( a q ) + H 2 O ( l ) ⇌ Fe ( H 2 O ) 5 ( OH ) 2 + ( a q ) + H 3 O + ( a q ) is 6.0 × 10−3.a. Calculate the pH of a 0.10-M solution of Fe(H2O)63+.b. Will a 1.0-M solution of iron(II) nitrate have a higher or lower pH than a 1.0-M solution of iron(III) nitrate? Explain.

(a)

Interpretation Introduction

Interpretation: The pH of the given solution is to be calculated and relation between the pH of iron(II) nitrate and that of iron(III) nitrate is to be stated.

Concept introduction: The pH of any solution depends upon the total [H+] concentration.  Metal ions with higher charge are more acidic than the metal ions with lower charge.

To determine: The pH of the given solution.

Explanation

Explanation

Given

The Ka value of the given solution is 6.0×103 .

Fe(H2O)6+3+H2OFe(H2O)5OH+2+H3O+Initial(M):0.1000Change(M):xxxEquilibrium(M):0

(b)

Interpretation Introduction

Interpretation: The pH of the given solution is to be calculated and relation between the pH of iron(II) nitrate and that of iron(III) nitrate is to be stated.

Concept introduction: The pH of any solution depends upon the total [H+] concentration.

Metal ions with higher charge are more acidic than the metal ions with lower charge.

To determine: The relation between the pH of iron(II) nitrate and that of iron(III) nitrate.

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