   # What concentration of NH 4 Cl is necessary to buffer a 0.52- M NH 3 solution at pH= 9.00? (K b for NH 3 = 1.8 × 10 −5 .) ### 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 101CWP
Textbook Problem
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## What concentration of NH4Cl is necessary to buffer a 0.52-M NH3 solution at pH= 9.00? (Kb for NH3 = 1.8 × 10−5.)

Interpretation Introduction

Interpretation: The necessary concentration of NH4Cl to buffer a 0.52MNH3 solution at the pH9.00 is to be calculated.

Concept introduction: The hydrogen ion concentration of the solution is known as pH of the solution.

It is the negative logarithm of Hydrogen ion concentration.

Buffer solution is the solution in which the concentration of Hydrogen ion remains same even with the addition of acid or base.

### Explanation of Solution

Explanation

Given

The value of equilibrium constant or base dissociation constant (Kb) for NH3 is 1.8×105 .

Ammonia is a base and NH4Cl is a weak acid of it that is also known as its salt.

Therefore, the concentration of its salt is calculated by the equation,

pH=pKb+log[salt][base]

Where,

• pKb is the negative logarithm of dissociation constant.
• [salt] is the concentration of salt.
• [acid] is the concentration of the acid.

The above equation is known as the Henderson-Hasselbalch equation.

The pKb that is a base dissociation constant is determined by the formula.

pKb=log(Kb)

Substitute the given value of Kb in the above equation.

pKb=log(Kb)=log(1

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