   # A buffered solution is made by adding 50.0 g NH 4 Cl to 1.00 L of a 0.75- M solution of NH 3 . Calculate the pH of the final solution. (Assume no volume change.) ### 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 38E
Textbook Problem
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## A buffered solution is made by adding 50.0 g NH4Cl to 1.00 L of a 0.75-M solution of NH3. Calculate the pH of the final solution. (Assume no volume change.)

Interpretation Introduction

Interpretation:

The mass of NH4Cl , concentration of NH3 and volume of a solution is given. The pH value of this solution is to be calculated.

Concept introduction:

The pOH value is the measure of OH ions. The relation between pOH and pKb is given by Henderson-Hassel Bach equation. According to this equation,

pOH=pKb+log[Conjugateacid][Weakbase]

To determine: The pH value of a solution made by adding 50g NH4Cl to 1.00L of NH3 solution

### Explanation of Solution

Explanation

To find the concentration of NH4Cl

Mass of NH4Cl is 50g .

The concentration of NH3 is 0.75M .

Volume of solution is 1.0L .

The molar mass of NH4Cl is 53.5.

Formula

The concentration of compound in a solution is calculated using the formula,

Concentrationofcompound=MassofcompoundMolarmassofcompound×Volumeofsolution

Substitute the values of mass, molar mass of NH4Cl and volume of solution.

Concentrationofcompound=MassofcompoundMolarmassofcompound×Volumeofsolution=5053.5×1=0.934M_

To find the pOH

The concentration of NH4Cl is 0.934M .

The concentration of NH3 is 0.75M .

The value of Kb for NH3 is 1.8×105 .

The pOH is calculated using the Henderson-Hassel Bach equation,

pOH=pKb+log[Conjugateacid][Weakbase] (1)

Where,

• pOH is the measure of OH ions

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