   # Calculate the pH of a solution that is 0.60 M HF and 1.00 M KF. ### 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 32E
Textbook Problem
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## Calculate the pH of a solution that is 0.60 M HF and 1.00 M KF.

Interpretation Introduction

Interpretation:

The concentration of HF and KF is given. The pH value of a solution of HF and KF is to be calculated.

Concept introduction:

The pH value is the measure of H+ ions. The relation between pH and pKa is given by Henderson-Hassel Bach equation. According to this equation,

pH=pKa+log[Base][Acid]

To determine: The pH value of a solution of 0.60M HF and 1.00M KF .

### Explanation of Solution

Explanation

Given

The concentration of HF is 0.60M .

The concentration of KF is 1.00M .

The value of Ka for HF is 7.2×104 .

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

pH=pKa+log[Base][Acid] (1)

Where,

• pH is the measure of H+ ions.
• pKa is the measure of acidic strength.
• [Base] is concentration of conjugate base.
• [Acid] is concentration of weak acid.

The formula of pKa is,

pKa=logKa

Where,

• Ka is acid equilibrium constant

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