   Chapter 16, Problem 16.112QP 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

Ionization of the first proton from H2SeO4 is complete (H2SeO4 is a strong acid); the acid-ionization constant for the second proton is 1.2 × 10−2. a What would be the approximate hydronium-ion concentration in 0.150 M H2SeO4 if ionization of the second proton were ignored? b The ionization of the second proton must be considered for a more exact answer, however. Calculate the hydronium-ion concentration in 0.150 M H2SeO4, accounting for the ionization of both protons.

(a)

Interpretation Introduction

Interpretation:

The hydronium ion concentration for the given cases has to be calculated.

1. (a) The hydronium ion concentration in 0.150 M H2SeO4 if ionization of second proton is ignored
2. (b) The hydronium ion concentration in 0.150 M H2SeO4 if ionization of both the protons are considered

Concept Introduction:

Strong acids undergo complete ionization whereas weak acid does not undergo ionization to full extent.

pH definition:

The pH of a solution is defined as the negative base-10 logarithm of the hydronium ion [H3O+] concentration.

pH=-log[H3O+]

On rearranging,

[H3O+] =10pH

Explanation

To Calculate: The hydronium ion concentration in 0.150 M H2SeO4 if ionization of second proton is ignored

Given data:

H2SeO4 is a strong acid.

Ionization of first proton is complete.

The second acid-ionization constant for the second proton is 1.2×102

The concentration of the acid = 0

(b)

Interpretation Introduction

Interpretation:

The hydronium ion concentration for the given cases has to be calculated.

1. (a) The hydronium ion concentration in 0.150 M H2SeO4 if ionization of second proton is ignored
2. (b) The hydronium ion concentration in 0.150 M H2SeO4 if ionization of both the protons are considered

Concept Introduction:

Strong acids undergo complete ionization whereas weak acid does not undergo ionization to full extent.

pH definition:

The pH of a solution is defined as the negative base-10 logarithm of the hydronium ion [H3O+] concentration.

pH=-log[H3O+]

On rearranging,

[H3O+] =10pH

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