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Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640

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BuyFindarrow_forward

Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640
Chapter 17.3, Problem 3RC
Textbook Problem
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Use Figure 17.10 to decide which indicator is best to use in the titration of NH3 with HCl shown in Figure 17.7.

  1. (a) crystal violet
  2. (b) thymol blue
  3. (c) methyl red
  4. (d) phenolphthalein

Interpretation Introduction

Interpretation:

The correct indicator should be identifed given the titation of ammonia (NH3) and hydrochloric acid (HCl) reaction, than using the figure 17.7.

Concept introduction:

Titration is a quantitative method to determine the quantity of an acid or base in a solution. This method is used to determine the concentration an acid in the solution by titrating it against a base. There are four types of acid-base titrations.

(1) Strong acid-Strong base, in this type of titration a strong acid is titrated against a strong base for example, HCl is titrated against NaOH .

(2) Strong acid-Weak base, in this type of titration a strong acid is titrated against a weak base for example, HCl is titrated against NH4OH .

(3) Weak acid-Strong base, in this type of titration a weak acid is titrated against a strong base for example, CH3COOH is titrated against NaOH .

(4) Weak acid-Weak base, in this type of titration a weak acid is titrated against a weak base for example, CH3COOH is titrated against NH4OH .

For weak base-strong acid titration the pH value can be calculated at various points before and after equivalence point.

The equilibrium established during the titration of NH3 with HCl . The equilibrium can be represented as,

NH3(aq)+ H3O+(aq)H2O(l)+NH4+(aq)

Here, the H3O+ ion are generated from HCl , and the reaction is written as,

HCl(aq)+H2O(l)H3O+(aq)+Cl(aq)

At equivalence point all the base will be neutralized, and there will be only NH4+ ion and H3O+ . The H3O+ will be produced due to the hydrolysis of NH4+ at equivalence point. The hydrolysis equilibrium is represented as,

NH4+(aq)+H2O(l) H3O+(aq)+NH3(aq)

By using the value of Ka for the NH4+ concentration of H3O+ can be calculated.

Ka=[H3O+][H2O][NH4+] (1)

As H3O+ ions are produced due to hydrolysis of NH4+ , the value of pH will be lower than 7 at equivalence point for the weak base-strong acid titrations.

Explanation of Solution

Reason for correct answer:

The pH titration for the given solution of NH3/HCl is given below.

There will be a reaction between NH3/HCl which can be represented in as

This titration are very useful to consider the tiration of a weak base with a strong acid, the figure (17.7) clearly explain the illustrate the (pH) curve for the titartion of 100.0mL of 0.001M for NH3 with 0.001M of HCl solution, the coresponding acid base reaction shown below.

The (pKa) reaction of ammonia and acid

NH3(aq)+ H3O+(aq)H2O(l)+NH4+(aq)Ka=5.6×1010

The The (pKb) reaction of ammonia and acid

NH3(aq)+ H3O+(aq)H2O(l)+NH4+(aq)Kb=1.8×105

[H3O+]=[NH4+][NH3]×Kb=1.8×105[H3O+]=KbHencepOH=pKb=log(1

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Chapter 17 Solutions

Chemistry & Chemical Reactivity
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