   # Aluminum ions react with the hydroxide ion to form the precipitate Al(OH) 3 ( s ), but can also react to form the soluble complex ion Al(OH) 4 − . In terms of solubility, Al(OH) 3 ( s ) will be more soluble in very acidic solutions as well as more soluble in very basic solutions. a. Write equations for the reactions that occur to increase the solubility of Al(OH) 3 ( s ) in very acidic solutions and in very basic solutions. b. Let’s study the pH dependence of the solubility of Al(OH) 3 ( s ) in more detail. Show that the solubility of Al(OH) 3 , as a function of [H + ], obeys the equation S = [ H + ] 3 K sp / K w 3 + K K w / [ H + ] where S = solubility = [Al 3+ ] + [Al(OH) 4 − ] and K is the equilibrium constant for Al(OH) 3 ( s ) + O H − ( a q ) ⇌ A l ( O H ) 4 − ( a q ) c. The value of K is 40.0 and K sp for Al(OH) 3 is 2 × 10 −32 . Plot the solubility of Al(OH) 3 in the pH range 4–12. ### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243

#### Solutions

Chapter
Section ### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243
Chapter 15, Problem 113MP
Textbook Problem
42 views

## Aluminum ions react with the hydroxide ion to form the precipitate Al(OH)3(s), but can also react to form the soluble complex ion Al(OH)4−. In terms of solubility, Al(OH)3(s) will be more soluble in very acidic solutions as well as more soluble in very basic solutions.a. Write equations for the reactions that occur to increase the solubility of Al(OH)3(s) in very acidic solutions and in very basic solutions.b. Let’s study the pH dependence of the solubility of Al(OH)3(s) in more detail. Show that the solubility of Al(OH)3, as a function of [H+], obeys the equation S   =   [ H + ] 3 K sp / K w 3   +   K K w / [ H + ] where S = solubility = [Al3+] + [Al(OH)4−] and K is the equilibrium constant for Al(OH) 3 ( s )   +   O H − ( a q )   ⇌   A l ( O H ) 4 − ( a q ) c. The value of K is 40.0 and Ksp for Al(OH)3 is 2 × 10−32. Plot the solubility of Al(OH)3 in the pH range 4–12.

(a)

Interpretation Introduction

Interpretation: The equations for the reactions that occur to increase the solubility of Al(OH)3 in very acidic and very basic solutions are to be stated. The solubility of Al(OH)3 as a function of [H+], obeys the given equation is to be shown. The solubility of Al(OH)3 in the pH range 412 is to be plotted.

Concept introduction: The constant Ksp is known as solubility product or solubility product constant. It is equilibrium constant and for a given solid, it has a particular value at a given temperature. However, the solubility is equilibrium position. The solubility product expression comprises of product of the ion concentrations.

### Explanation of Solution

Explanation

To determine: The equations for the reactions that occur to increase the solubility of Al(OH)3 in very acidic and very basic solutions.

The equations are given below.

Aluminum ions react with the hydroxide ion to form precipitate Al(OH)3, but it also react to form the soluble complex ion Al(OH)4. The precipitate is more soluble in very acidic and very basic solutions.

The equations for the reactions that occur to increase the solubility of Al(OH)3 in very acidic solution is,

Al(OH)3(s)

(b)

Interpretation Introduction

Interpretation: The equations for the reactions that occur to increase the solubility of Al(OH)3 in very acidic and very basic solutions are to be stated. The solubility of Al(OH)3 as a function of [H+], obeys the given equation is to be shown. The solubility of Al(OH)3 in the pH range 412 is to be plotted.

Concept introduction: The constant Ksp is known as solubility product or solubility product constant. It is equilibrium constant and for a given solid, it has a particular value at a given temperature. However, the solubility is equilibrium position. The solubility product expression comprises of product of the ion concentrations.

(c)

Interpretation Introduction

Interpretation: The equations for the reactions that occur to increase the solubility of Al(OH)3 in very acidic and very basic solutions are to be stated. The solubility of Al(OH)3 as a function of [H+], obeys the given equation is to be shown. The solubility of Al(OH)3 in the pH range 412 is to be plotted.

Concept introduction: The constant Ksp is known as solubility product or solubility product constant. It is equilibrium constant and for a given solid, it has a particular value at a given temperature. However, the solubility is equilibrium position. The solubility product expression comprises of product of the ion concentrations.

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