   Chapter 15, Problem 51E

Chapter
Section
Textbook Problem

# Which of the following mixtures would result in buffered solutions when 1.0 L of each of the two solutions are mixed?a. 0.1 M KOH and 0.1 M CH3NH3Clb.0.1M KOH and 0.2 M CH3NH2c. 0.2 M KOH and 0.1 M CH3NH3Cld. 0.1 M KOH and 0.2 M CH3NH3Cl

Interpretation Introduction

Interpretation:

The mixtures that would result in buffered solution are to be identified from the given list.

Concept introduction:

A solution that contains mixture of a weak acid and its conjugate base or weak base and its conjugate acid is known as buffer solution. This solution resists any gross change in pH .

Explanation

Explanation

(a)

To identify: If the mixture of 0.1M KOH and 0.1M CH3NH3Cl would result in a buffered solution.

The mixture of 0.1M KOH and 0.1M CH3NH3Cl would not result in a buffered solution.

A reaction of KOH and CH3NH3Cl is said to be buffer, if CH3NH3+ (acid) and CH3NH2 (base) present at the end of reaction.

KOH is a strong base whereas, CH3NH3Cl is a salt of strong acid. The reaction is,

CH3NH3++OHCH3NH2+H2O

Both KOH and CH3NH3Cl have same concentration. As OH reacts completely, no CH3NH3+ is left after completion of reaction. Hence, it is not a buffer solution.

(b)

KOH is a strong base, whereas CH3NH2 is also a base. Hence, it will not form a buffer solution.

(c)

A reaction of KOH and CH3NH3Cl is said to be buffer, if CH3NH3+ (acid) and CH3NH2 (base) present at the end of reaction

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