   # The enthalpy of neutralization for the reaction of a strong acid with a strong base is −56 kJ/mol water produced. How much energy will be released when 200.0 mL of 0.400 M HNO 3 is mixed with 150.0 mL of 0.500 M KOH? ### 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 7, Problem 99AE
Textbook Problem
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## The enthalpy of neutralization for the reaction of a strong acid with a strong base is −56 kJ/mol water produced. How much energy will be released when 200.0 mL of 0.400 M HNO3 is mixed with 150.0 mL of 0.500 M KOH?

Interpretation Introduction

Interpretation: For strong acid with strong base reaction, the enthalpy of neutralization given as -56 kJ/mol. Amount of energy released to be calculated.

Concept introduction

Standard enthalpy of neutralization: The enthalpy change found when one equivalent of both an acid and base undergo neutralization to form salt and water.

Molarity: Molarity defined as number of moles of solute present in one litre of the solution.

### Explanation of Solution

Explanation

Given data:

Standard enthalpy change for strong acid with strong base reaction has given as -56 kJ/mol.

Quantity of  HNO3=200 mL

Quantity of  KOH=150mL

Concentration of  HNO3=0.4 M

Concentration of  KOH=0.5M

Calculate amount of energy released for given reaction as follows –

0.2000 L×(0.400 molHNO3L)×(56 kJ heat releasedmolHNO3)

= 4.5 kJ if HNO3 boundary

0.1500 L×(0

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