   # What is the pH of the solution that results from adding 30.0 mL of 0.100 M NaOH to 45.0 mL of 0.100 M acetic acid? (a) 2.87 (b) 5.05 (c) 7.00 ### 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 17.1, Problem 1RC
Textbook Problem
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## What is the pH of the solution that results from adding 30.0 mL of 0.100 M NaOH to 45.0 mL of 0.100 M acetic acid? (a) 2.87 (b) 5.05 (c) 7.00

Interpretation Introduction

Interpretation:

The value of pH is to be calculated for the given mixture which contains 30mL sodium hydroxide (0.003molL1) and 45mL sodium hydroxide (0.045molL1) solutions.

Concept introduction:

A buffer is defined as a solution which does not show any change in its pH values on addition of small amount of acid or base. There are two types of buffer solutions, (1) Acidic Buffer and (2) Basic Buffer.

Acidic Buffer is a solution which has the pH value below 7 . An acidic buffer is prepared by mixing a weak acid with its conjugate base. For example a mixture of weak acid CH3COOH and its conjugate base CH3COO gives a acidic buffer.

CH3COOH(aq.)+ H2O(l)H3O+(aq.)+ CH3COO1(aq.)

Basic Buffer is a solution which has the pH value above 7 . A basic buffer is prepared by mixing a weak base with its conjugate acid. For example a mixture of weak base NH4OH and its conjugate acid NH4+ gives a baisc buffer.

NH4OH(aq.)NH4+(aq.)+ OH1(aq.)

### Explanation of Solution

The pH value calculation for the given solution of NaOH/CH3COOH is given below.

There will be a reaction between CH3COOH  and NaOH  which can be represented in an

ICE table (1).

VolumeofNaOH=30mLMolarofNaOH=0.100MVolumeofCH3COOH=45mLMolarofCH3COOH=0.100MEquationCH3COOH(aq)+NaOH(aq)H2O(l)+CH3COONa(aq)Initial(mol)0.00450.0030Change(mol)0

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