   # What are the equilibrium concentrations of acetic acid, the acetate ion, and H 3 O + for a 0.10 M solution of acetic acid (K 2 = 1.8 × 10 −5 )? What is the pH of the solution? ### 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 16.7, Problem 2CYU
Textbook Problem
1 views

## What are the equilibrium concentrations of acetic acid, the acetate ion, and H3O+ for a 0.10 M solution of acetic acid (K2 = 1.8 × 10−5)? What is the pH of the solution?

Interpretation Introduction

Interpretation:

Equilibrium concentration of acetic acid, acetate ion, H3O+and pHof 0.10M solution of acetic acid has to be determined

Concept introduction:

The pHof a solution of acetic acid can be calculated by using the hydronium ion concentration by using the expression, pH=logH3O+.

Hydronium ion concentration is calculated by considering the equilibrium conditions and from the value of acid dissociation constant.

The concentration of acetic acid and acetate ion is determined by using equilibrium condition The concentration of acetate ion and hydronium ion is equal at equilibrium according to the reaction stoichiometry.

Equilibrium constants:

The equilibrium constant is used to quantitative measurement of the strength of the acid and bases in the water.

Ka is an acid constant for equilibrium reactions.

HA + H2OH3O++ A-Ka[H3O+][A-][HA]

Kb is a base constant for equilibrium reaction.

BOH + H2OB++ OH-Ka[B+][OH-][BOH]

### Explanation of Solution

Given data is as follows:

The initial concentration of the acetic acid solution is0.10M.

The acid dissociation constant Ka of acetic acid is 1.8×105.

The ICE table for the dissociation of acetic acid is given below,

EquilibriumCH3COOHaqCH3COOaq+H3O+aqInitialM0.1000ChangeMx+x+xEquilibriumM0.10xxx

From ICE table the expression for Ka;

Ka=CH3COOH3O+CH3COOH

Substituting equilibrium concentrations for acetate ion, hydronium ion, and acetic acid;

Ka=x20.1x

Substituting the value of acid dissociation constant Ka in the above equation,

1

### Still sussing out bartleby?

Check out a sample textbook solution.

See a sample solution

#### The Solution to Your Study Problems

Bartleby provides explanations to thousands of textbook problems written by our experts, many with advanced degrees!

Get Started

Find more solutions based on key concepts
What is the name of the element in Group 4A and Period 5?

General Chemistry - Standalone book (MindTap Course List)

Vitamin C deficiency symptoms include: red spots. loose teeth. anemia. all of the above.

Nutrition: Concepts and Controversies - Standalone book (MindTap Course List)

6.45 Define the term shielding.

Chemistry for Engineering Students

14-38 Show how to convert this alcohol to compounds (a) and (b).

Introduction to General, Organic and Biochemistry

Describe two ways an atom can become excited.

Horizons: Exploring the Universe (MindTap Course List)

What is a life cycle?

Biology: The Dynamic Science (MindTap Course List)

What is the chief chemical property of ethers?

Chemistry for Today: General, Organic, and Biochemistry

Find the scalar product of the vectors in Figure P7.7. Figure P7.7

Physics for Scientists and Engineers, Technology Update (No access codes included)

How are the heaviest elements (uranium or gold) thought to be formed?

Oceanography: An Invitation To Marine Science, Loose-leaf Versin 