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Introductory Chemistry: A Foundati...

9th Edition
Steven S. Zumdahl + 1 other
ISBN: 9781337399425

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BuyFindarrow_forward

Introductory Chemistry: A Foundati...

9th Edition
Steven S. Zumdahl + 1 other
ISBN: 9781337399425
Textbook Problem
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. Despite HCI’s being a strong acid, the pH of 1.00 × 10 7 M HCI is not exactly 7.00. Can you suggest a reason why?

Interpretation Introduction

Interpretation:

Why the pH of 1.00×107 M HCl is not exactly 7.00 should be explained.

Concept Introduction:

The concentration of hydrogen ions in a solution determines the acidity of a solution. If concentration of hydrogen ion is more than the solution is more acetic, if it is low, solution is less acidic.

The pH of solution is defined as negative log of hydrogen ion concentration thus, it can be calculated as follows:

pH=logH+

Here, H+ is concentration of hydrogen ion.

Similarly, pOH of a solution is defined as negative log of hydroxide ion concentration thus, it can be calculated as follows:

pOH=logOH

Here, OH is concentration of hydroxide ion.

pH and pOH of a solution are related to each other as follows:

pH+pOH=14.

Explanation

If the concentration of HCl is small such as 1.00×107 M, along with the hydrogen ion concentration from HCl, the hydrogen ion concentration from water is also considered which is also approximately 1.00×107 M because water is neutral with pH 7.

For such cases, the total hydrogen ion concentration will be sum of hydrogen ion concentration from HCl and that from water.

HClH++Cl

H2OH++OH

Thus, total hydrogen ion concentration will be:

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