   Chapter 16.6, Problem 16.5CC 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

You add 1.5 mL of 1 M HCl to each of the following solutions. Which one will show the least change of pH? a 15 mL of 0.1 M NaOH b 15 mL of 0.1 M HC2H3O2 c 30 mL of 0.1 M NaOH and 30 mL of 0.1 M HC2H3O2 d 30 mL of 0.1 M NaOH and 60 mL of 0.1 M HC2H3O2

Interpretation Introduction

Interpretation:

Among the given solutions, which solution will show least change of pH on addition of 1.5 mL of 1 M HCl has to be identified

Concept Information:

pH definition:

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

pH=-log[H+]

To Identify: Among the given solutions, which solution will show least change of pH on addition of 1.5 mL of 1 M HCl

Explanation

(a)

Addition of 1.5 mL of 1 M HCl to 15 mL of 0.1 M NaOH

HCl is a strong acid and NaOH is a strong base.

Hence, addition of 1.5 mL of 1 M HCl to 15 mL of 0.1 M NaOH neutralizes the solution by giving a solution of Sodium chloride salt.

Thus, the pH of the original solution alters from very basic to neutral (pH = 7) after the addition of HCl .

(b)

Addition of 1.5 mL of 1 M HCl to 15 mL of 0.1 M HC2H3O2

Acetic acid is weak acid. Hence, by the addition of HCl , the solution of weak acid (acetic acid), changes to strongly acidic solution

(c)

Addition of 1.5 mL of 1 M HCl to 30 mL of 0.1 M NaOH and 30 mL of 0.1 M HC2H3O2

The amounts of NaOH and HC2H3O2   are equal

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