   Chapter 15, Problem 88QAP ### Introductory Chemistry: A Foundati...

9th Edition
Steven S. Zumdahl + 1 other
ISBN: 9781337399425

#### Solutions

Chapter
Section ### Introductory Chemistry: A Foundati...

9th Edition
Steven S. Zumdahl + 1 other
ISBN: 9781337399425
Textbook Problem
2 views

# 88. Suppose that 27.34 mL of standard 0.1021 M NaOH is required to neutralize 25.00 mL of an unknown H2SO4 solution. Calculate the molarily and the normality of the unknown solution.

Interpretation Introduction

Interpretation:

The normality and molarity of the unknown solution of H2SO4 is to be calculated.

Concept Introduction:

Neutralization is the process in which an acid and base react with each other to give salt and water. The general reaction of acid and base is represented as:

AH+BOHAB+H2O

The normality of a solution is defined as the gram equivalent weight of a solute dissolved in one liter of the solution.

Molarity of a solution is defined as the number of moles of solute dissolved in one liter of the solution.

Explanation

The molarity of the given NaOH solution is 0.1021M.

The volume of NaOH solution required to neutralize unknown solution of H2SO4 is 27.34mL.

The volume of unknown solution of H2SO4 is 25.00mL.

The equivalence factor of H2SO4 is 2eqmol1.

The neutralization reaction between H2SO4 and NaOH is represented as:

H2SO4+2NaOHNa2SO4+2H2O

The relation between the volume of NaOH and H2SO4 required for neutralization reaction is represented as,

MaVa=2MbVb        (1)

Where,

• Ma represents the normality of the H2SO4.
• Mb represents the normality of the NaOH.
• Va represents is the volume of H2SO4.
• Vb represents is the volume of NaOH.

Rearrange the equation (1) for the value of Ma

### 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 