   # A 2.5 × 10 −3 M solution of an unknown acid has a pH of 3.80 at 25 °C. (a) What is the hydronium ion concentration of the solution? (b) Is the acid a strong acid, a moderately weak acid ( K a of about 10 −5 ), or a very weak acid ( K a of about 10 −10 )? ### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640

#### Solutions

Chapter
Section ### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640
Chapter 16, Problem 47PS
Textbook Problem
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## A 2.5 × 10−3 M solution of an unknown acid has a pH of 3.80 at 25 °C. (a) What is the hydronium ion concentration of the solution? (b) Is the acid a strong acid, a moderately weak acid (Ka of about 10−5), or a very weak acid (Ka of about 10−10)?

(a)

Interpretation Introduction

Interpretation: The hydronium ion concentration in the unknown acid solution has to be identified.

Concept introduction:

The pH value of acid gives the concentration of hydrogen ion. The expression used for the calculation of hydrogen ion concentration is given as pH=log[H+].

### Explanation of Solution

It is given that pH of an unknown acid is 3.80

pH=log[H+]3.80=log[H+]

From the above equation,

[H+]=10(3

(b)

Interpretation Introduction

Interpretation: The ionization constant (Ka) of an unknown acid has to be calculated. and the acid is a strong acid or a moderately weak acid or very weak acid also to be identified.

Concept introduction:

The acid dissociation constant or acid ionization constant of unknown acid can be determined by using the pH value of acid (which gives the concentration of hydrogen ion) and from the given concentration of unknown acid.

The pH value of acid gives the concentration of hydrogen ion. The expression used for the calculation of hydrogen ion concentration is given as pH=log[H+]

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