   Chapter 16, Problem 94GQ

Chapter
Section
Textbook Problem

The butylammonium ion, C4H9NH3+, has a Ka of 2.3 × 10−11.C4H9NH3+(aq) + H2O(ℓ) ⇄ H3O+(aq) + C4H9NH2(aq) a) Calculate Kb for the conjugate base, C4H9NH2 (butyl amine). b) Place the butylammonium ion and its conjugate base in Table 16.2. Name an acid weaker than C4H9NH3+ and a base stronger than C4H9NH3. c) What is the pH of a 0.015M solution of butylammonium chloride?

(a)

Interpretation Introduction

Interpretation:

Kb has to be calculated for the conjugate base (C4H9NH2, butyl amine)

Concept Introduction:

Equilibrium constants:

The equilibrium constant is used to quantitative measurement of the strength of the acid and bases in the water.

Ka is an acid constant for equilibrium reactions.

HA + H2OH3O++ A-Ka[H3O+][A-][HA]

Kb is a base constant for equilibrium reaction.

BOH + H2OB++ OH-Ka[B+][OH-][BOH]

Ion product constant for wter  Kw= [H3O+][OH-]       =1.00×10-14 pH = -log[H3O+]pOH= -log[OH-]

Relation between pH and pOH

pH + pOH =14

Explanation

According to the Brown stead –Lowry theory the compound which is accepts a proton to be considered as a base.

A weak base accepts a proton from water molecules producing hydroxide ions in water.

The Ka of 2.3× 10-11

Ka×Kb = KwKbKwKaKw= 1.0×10-14Ka = 2

(b)

Interpretation Introduction

Interpretation:

Compound should be Named for an acid weaker than C4H9NH3+ and a base stronger than C4H9NH2.

Concept Introduction:

Equilibrium constants:

The equilibrium constant is used to quantitative measurement of  the strength of the acid and bases in the water .

Ka an acid constant for equilibrium reactions.

HA + H2OH3O++ A-Ka[H3O+][A-][HA]

Kb is base constant for equilibrium reaction.

BOH + H2OB++ OH-Ka[B+][OH-][BOH]

Ion product constant for wter  Kw= [H3O+][OH-]       =1.00×10-14 pH = -log[H3O+]pOH= -log[OH-]

Relation between pH and pOH

pH + pOH =14

(c)

Interpretation Introduction

Interpretation:

The pH has be calculated for 0.015M solution of butylammonium chloride?

Concept Introduction:

Equilibrium constants:

The equilibrium constant is used to quantitative measurement of  the strength of the acid and bases in the water .

Ka is an acid constant for equilibrium reactions.

HA + H2OH3O++ A-Ka[H3O+][A-][HA]

Kb is a base constant for equilibrium reaction.

BOH + H2OB++ OH-Ka[B+][OH-][BOH]

Ion product constant for wter  Kw= [H3O+][OH-]       =1.00×10-14 pH = -log[H3O+]pOH= -log[OH-]

Relation between pH and pOH

pH + pOH =14

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