   Chapter 16, Problem 16.69QP General Chemistry - Standalone boo...

11th Edition
Steven D. Gammon + 7 others
ISBN: 9781305580343

Solutions

Chapter
Section General Chemistry - Standalone boo...

11th Edition
Steven D. Gammon + 7 others
ISBN: 9781305580343
Textbook Problem

Calculate the degree of ionization of a 0.75 M HF (hydrofluoric acid); b the same solution that is also 0.12 M HCl.

(a)

Interpretation Introduction

Interpretation:

The degree of ionization of the given acid solutions has to be calculated

Concept Introduction:

The equilibrium expression for the weak acid is given below.

Ka=[H+][A-][HA]

Where,

Ka is acid ionization constant,

[H+] is concentration of hydrogen ion

[A-] is concentration of acid anion

[HA] is concentration of the acid

Degree of ionization (α) is the amount of reactant that undergoes ionization in the reaction.

Explanation

To Calculate: The degree of ionization of 0.75 M HF

Given data:

The concentration of hydrofluoric acid (HF)  = 0.75 M

Degree of ionization:

Construct the equilibrium table, for the given solution.

Let x be the unknown concentration

 HF   +   H2O  ⇌   H3O+   +   F− Initial (M) 0.75 −x 0.75-x 0.00 0.00 Change (M) +x +x Equilibrium (M) x x

The Ka for hydrofluoric acid is 6.8×104

Substitute into the equilibrium-constant equation.

Ka =[H3O+][F-][HF] =(x)2(0

(b)

Interpretation Introduction

Interpretation:

The degree of ionization of the given acid solutions has to be calculated

Concept Introduction:

The equilibrium expression for the weak acid is given below.

Ka=[H+][A-][HA]

Where,

Ka is acid ionization constant,

[H+] is concentration of hydrogen ion

[A-] is concentration of acid anion

[HA] is concentration of the acid

Degree of ionization (α) is the amount of reactant that undergoes ionization in the reaction.

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