   Chapter 14, Problem 115E

Chapter
Section
Textbook Problem

# Given that the Ka value for acetic acid is 1.8 × 10−5 and the Ka value for hypochlorous acid is 3.5 × 10−8, which is the stronger base, OCl− or C2H3O2−?

Interpretation Introduction

Interpretation: The stronger base among the given species is to be identified.

Concept introduction: A molecule or an ion that is capable of donating a proton or accepting an electron pair in a chemical reaction is known as an acid.

A substance that reacts with acids, leading to the production of salts is known as a base.

The acidic strength increases with an increase in the Ka value.

When an acid donates a proton, the species left is termed as a conjugate base.

Explanation

Explanation

To identify: The stronger base among the given species.

Acetic acid is a stronger acid than hypochlorous acid.

Given

The Ka value for acetic acid (CH3COOH) is 1.8×105 .

The Ka value for hypochlorous acid (HOCl) is 3.5×108 .

The acidic strength increases with an increase in the Ka value.

Therefore, CH3COOH is a stronger acid than HOCl .

OCl is a stronger base than C2H3O2

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