# Consider the following mathematical expressions. a. [H + ] = [HA] 0 b. [H + ] = ( K a × [HA] 0 ) 1/2 c. [OH − ] = 2[B] 0 d. [OH − ] = ( K b × [B] 0 ) 1/2 For each expression, give three solutions where the mathematical expression would give a good approximation for the [H + ] or [OH − ]. [HA] 0 and [B] 0 represent initial concentrations of an acid or a base.

### Chemistry: An Atoms First Approach

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

Chapter
Section

### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243
Chapter 13, Problem 31Q
Textbook Problem
5 views

## Consider the following mathematical expressions.a. [H+] = [HA]0b. [H+] = (Ka × [HA]0)1/2c. [OH−] = 2[B]0d. [OH−] = (Kb × [B]0)1/2For each expression, give three solutions where the mathematical expression would give a good approximation for the [H+] or [OH−]. [HA]0 and [B]0 represent initial concentrations of an acid or a base.

(a)

Interpretation Introduction

Interpretation: Three solutions for each of the given mathematical expression that would give a good approximation for the [H+] or [OH] are to be stated.

Concept introduction: The state when the reactants involved in a chemical reaction and the products formed in the reaction exist in concentrations having no further tendency to change is known as an equilibrium state of the reaction.

The equilibrium constant for the dissociation reaction of a given acid is known as the acid dissociation constant and is denoted by the symbol, Ka .

The equilibrium constant for the dissociation reaction of a given base is known as the base dissociation constant and is denoted by the symbol, Kb .

### Explanation of Solution

To determine: Three solutions for the given mathematical expression, [H+]=[HA]0

For the given case, the strong acid solutions such as 0.1M HNO3 , 1.0×1010M HCl and 0.02M HClO4 would give a good approximation for the [H+]

(b)

Interpretation Introduction

Interpretation: Three solutions for each of the given mathematical expression that would give a good approximation for the [H+] or [OH] are to be stated.

Concept introduction: The state when the reactants involved in a chemical reaction and the products formed in the reaction exist in concentrations having no further tendency to change is known as an equilibrium state of the reaction.

The equilibrium constant for the dissociation reaction of a given acid is known as the acid dissociation constant and is denoted by the symbol, Ka .

The equilibrium constant for the dissociation reaction of a given base is known as the base dissociation constant and is denoted by the symbol, Kb .

(c)

Interpretation Introduction

Interpretation: Three solutions for each of the given mathematical expression that would give a good approximation for the [H+] or [OH] are to be stated.

Concept introduction: The state when the reactants involved in a chemical reaction and the products formed in the reaction exist in concentrations having no further tendency to change is known as an equilibrium state of the reaction.

The equilibrium constant for the dissociation reaction of a given acid is known as the acid dissociation constant and is denoted by the symbol, Ka .

The equilibrium constant for the dissociation reaction of a given base is known as the base dissociation constant and is denoted by the symbol, Kb .

(d)

Interpretation Introduction

Interpretation: Three solutions for each of the given mathematical expression that would give a good approximation for the [H+] or [OH] are to be stated.

Concept introduction: The state when the reactants involved in a chemical reaction and the products formed in the reaction exist in concentrations having no further tendency to change is known as an equilibrium state of the reaction.

The equilibrium constant for the dissociation reaction of a given acid is known as the acid dissociation constant and is denoted by the symbol, Ka .

The equilibrium constant for the dissociation reaction of a given base is known as the base dissociation constant and is denoted by the symbol, Kb .

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