   Chapter 16, Problem 46PS

Chapter
Section
Textbook Problem

A 0.10 M solution of chloroacetic acid, CICH2CO2H, has a pH of 1.95. Calculate Ka for the acid.

Interpretation Introduction

Interpretation:

Acid ionization constant (Ka) of chloroacetic acid has to be calculated.

Concept introduction:

The acid dissociation constant or acid ionization constant of chloroacetic acid can be determined by using the pH value of chloroacetic acid (which gives the concentration of hydrogen ion) and from the given concentration of chloroacetic acid.

Explanation

Given data,

The pH of chloroacetic acid is 1.95

The concentration of chloroacetic acid is 0.10M

Calculate the acid dissociation constant (Ka) of the acid as follows -

It is known that pH=log[H+]

From the above equation, the concentration of H+ can be calculated to be

[H+]=0.0112

The equation for the equilibrium of dissociation of chloroacetic acid is represented as below,

EquilibriumClCH2COOH(aq)ClCH2COO(aq)+H+(aq)Initial(M)0.1000Change(M)x+x+xEquilibrium(M)0

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