   # What is the pH after 25.0 ml of 0.100 M NaOH has been added to 50.0 ml of 0.100 M HCl? (a) 1.00 (b) 1.48 (c) 7.00 (d) 13.00 ### 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 17.3, Problem 1RC
Textbook Problem
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## What is the pH after 25.0 ml of 0.100 M NaOH has been added to 50.0 ml of 0.100 M HCl? (a) 1.00 (b) 1.48 (c) 7.00 (d) 13.00

Interpretation Introduction

Interpretation:

The value of pH is to be calculated for the resulting solution obtained by adding 25mL of 0.100M sodium hydroxide (NaOH) and 50.0mL 0.100 M (HCl) solution.

Concept introduction:

A buffer solution is defined as a solution which does not show any change in its pH values on the 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 an 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 basic buffer.

NH4OH(aq.)NH4+(aq.)+ OH1(aq.)

### Explanation of Solution

The pH value for the resulting obtained by adding 25mL 0.12 M hydrochloric acid and 25mL 0.43 M ammonia solution is calculated below.

Given:

Given the data Volume ofNaOHsoultion=25mLMolarofNaOHsoultion=0.100nNaOH= 0.1×0.025L=0.0025molnHCl= 0.1×0.050L=0.0050molThe buffer reactionNaOH+HClNaCl+H2O

The ICE table (1) is as follows,

EquationHCl(aq)+NaOH(aq)NaCl(aq)+H2O(l)Initial(mol)0.0050.00250Change(mol)0.00250.00250.0025Afterreaction(mol)0

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