   Chapter 14, Problem 165CWP

Chapter
Section
Textbook Problem

# Consider a 0.67-M solution of C2H5NH2 (Kb = 5.6 × 10−4).a. Which of the following are major species in the solution?i. C2H5NH2ii. H+iii. OH−iv. H2Ov. C2H5NH3+b. Calculate the pH of this solution.

Interpretation Introduction

Interpretation: The major species present in the given 0.67M C2H5NH2 solution and the pH of the given solution is to be stated.

Concept introduction: Ethyl amine (C2H5NH2) is an electron rich species and acts as a nucleophile. In aqueous solution, Ethyl; amine acts as a weak base dissociating partially and slowly.

To determine: The major species of 0.67M C2H5NH2 solution.

Explanation

Explanation

The major species in aqueous solution is C2H5NH3+ and OH .

Ethyl amine dissociates into ions partially and slowly because of weak basic nature.

C2H5NH2+H2OC2H5NH3++OH

The aqueous solution of Ethyl amine contains C2H5NH3+ and OH as major species.

The value of [OH] at equilibrium is 0.019092M_ .

The ICE (Initial Change Equilibrium) table of the dissociation of Ethyl amine is,

C2H5NH2+H2OC2H5NH3++OHInitial(M):0.6700Change(M):xxxEquilibrium(M):0.67xMxx

The base dissociation constant for the above reaction is,

Kb=[C2H5NH3+][OH][C2H5NH2]

Substitute the values of concentration of reactants and products from the ICE table to the above Kb formula

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