   # What quantity (moles) of HCl( g ) must be added to 1.0 L of 2.0 M NaOH to achieve a pH of 0.00? (Neglect any volume changes.) ### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243

#### Solutions

Chapter
Section ### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243
Chapter 14, Problem 88AE
Textbook Problem
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## What quantity (moles) of HCl(g) must be added to 1.0 L of 2.0 M NaOH to achieve a pH of 0.00? (Neglect any volume changes.)

Interpretation Introduction

Interpretation:

The quantity of HCl that must be added to 1.0L of 2.0M NaOH to achieve a pH of 0.00 is to be calculated.

Concept introduction:

The pH of a solution is calculated by the formula,

pH=log[H+]

### Explanation of Solution

Explanation

To find the moles of NaOH present

Given

Molarity of NaOH is 2.0M .

Volume is 1.0L .

The number of moles is calculated by the formula,

Numberofmoles=Molarity×Volume(L)

Substitute the value of the given molarity of NaOH and the volume in the above expression.

Numberofmoles=2.0M×1.0L=2.0mol_

To find the [H+]

The given value of pH is 0.00 .

The pH of a solution is calculated by the formula,

pH=log[H+]

Rearrange the above expression to calculate the value of [H+] .

[H+]=10pH

Substitute the given value of pH in the above expression.

[H+]=100.0=1.0M_

To find the quantity of HCl that must be added to 1.0L of 2.0M NaOH to achieve a pH of 0

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