   # Calculate the pH after 0.020 mole of HCl is added to 1.00 L of each of the four solutions in Exercise 22. ### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243

#### Solutions

Chapter
Section ### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243
Chapter 14, Problem 26E
Textbook Problem
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## Calculate the pH after 0.020 mole of HCl is added to 1.00 L of each of the four solutions in Exercise 22.

(a)

Interpretation Introduction

Interpretation: The pH of the resulting solution when 0.020 moles of HCl is added to 1.00L of given solutions.

Concept Introduction: The value of pH for weak acids and buffer solution is calculated by the Henderson-Hasselbalch equation.

pH=pKa+log[Base][Acid]

To determine: The pH of the solution when 0.020 moles of HCl is mixed with 1L of 0.100MHONH2 .

### Explanation of Solution

Explanation

At 0.020 moles addition of HCl to the 1L of 0.100MHONH2 the concentration of hydroxylamine (HONH3+) ion at equilibrium is calculated by using reaction stoichiometric coefficients.

HONH2+HClHONH3+NumberofMolesbeforethereaction0.1000.0200NumberofMolesafterthereaction0.0800.020

The value of concentration of a species is calculated by the formula.

Concentration=NumberofmolesVolumeofsolution

The concentration of base (HONH2) is calculated as,

[HONH2]=0.081.00L[HONH2]=0.08M

The concentration of weak conjugate acid (HONH3+) is calculated as,

[HONH3+]=0.021.00L

The buffer produced by the combination of base HONH2 and its conjugate acid HONH3+ is basic in nature.

The value of Kb for HONH2 is 1

(b)

Interpretation Introduction

Interpretation: The pH of the resulting solution when 0.020 moles of HCl is added to 1.00L of given solutions.

Concept Introduction: The value of pH for weak acids and buffer solution is calculated by the Henderson-Hasselbalch equation.

pH=pKa+log[Base][Acid]

To determine: The pH of the solution when 0.020 moles of HCl is mixed with 1L of 0.100MHONH3Cl .

(c)

Interpretation Introduction

Interpretation: The pH of the resulting solution when 0.020 moles of HCl is added to 1.00L of given solutions.

Concept Introduction: The value of pH for weak acids and buffer solution is calculated by the Henderson-Hasselbalch equation.

pH=pKa+log[Base][Acid]

To determine: The pH of the solution when 0.020 moles of HCl is mixed with 1L of pure water.

(d)

Interpretation Introduction

Interpretation: The pH of the resulting solution when 0.020 moles of HCl is added to 1.00L of given solutions.

Concept Introduction: The value of pH for weak acids and buffer solution is calculated by the Henderson-Hasselbalch equation.

pH=pKa+log[Base][Acid]

To determine: The pH of the solution when 0.020 moles of HCl is mixed with 1L of mixture containing 0.100MHONH2 and 0.100MHONH3Cl .

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