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Chemistry: An Atoms First Approach

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

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BuyFindarrow_forward

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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Chapter 14 Solutions

Chemistry: An Atoms First Approach
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Ch. 14 - What are the major species in solution after...Ch. 14 - A friend asks the following: Consider a buffered...Ch. 14 - Mixing together solutions of acetic acid and...Ch. 14 - Could a buffered solution be made by mixing...Ch. 14 - Sketch two pH curves, one for the titration of a...Ch. 14 - Sketch a pH curve for the titration of a weak acid...Ch. 14 - You have a solution of the weak acid HA and add...Ch. 14 - You have a solution of the weak acid HA and add...Ch. 14 - The common ion effect for weak acids is to...Ch. 14 - Consider a buffer solution where [weak acid] ...Ch. 14 - A best buffer has about equal quantities of weak...Ch. 14 - Consider the following pH curves for 100.0 mL of...Ch. 14 - An acid is titrated with NaOH. 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